Answers
The but-2-ene is a molecule with four carbons and the middle bond, (the second one) is a double-bond.
So, its structure is H₃C-CH=CH-CH₃.
However, the double bond makes two possible isomers, the "e" and "z":
The double bond, differently from the single bond, does not rotate, so these structures are not the same.
In the left one, the carbon groups have higher priority, and they are in alternating sides, bottom and top, and so it is called the E isomer.
In the right one, the carbon groups are on the same side, so it is called the Z isomer.
Related Questions
What is the wavelength of light with a frequency of 3.215 x 10^15 s-¹?
A. 9.325 x 10^-8m
B. 3.110 x 10^-16m
C. 1.072 x 10^7 m
D. 9.639 x 10^23m
Answers
The wavelength of the light will be 9.63 × 10²³ m .The wavelength of the wave is calculated using the frequency formula.
The quantity of cycles finished in a certain amount of time is known as frequency. It also indicates the number of crests that pass past a specific position in a unit of time. It is often referred to as the reciprocal of time. Hertz are used to express frequency (Hz). The frequency of the wave is calculated using the frequency formula.
The total number of times a repeated event occurs in a unit of time is known as its frequency. Depending on the quantities known, various frequency formulas exist to calculate frequency. The terms frequency (f), time period (T), wave speed (V), and wavelength () are all found using the formula for the frequency of a wave.
We know that ,
Frequency= Speed of light/ wavelength
Wavelength= Frequency × Speed of light
= 3.215 ×10¹⁵ × 2.997× 10⁸
= 9.639 × 10²³ m
The wavelength will be obtained by frequency -wavelength formula a and it will come as 9.63 × 10²³ m .
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The frequency of a wave is 1.2 x 10° Hz. What is its wavelength? What kind of wave is this?
Answers
Answer: wavelength= ............
Explanation:
Are all covalent molecules soluble in water ?
Answers
Explanation:
determining which kind of elements are soluble, especially covalent molecules. Chemical balances, no matter in bonds. chemical balances, physical balances are reasons why.
Determine the mass of the sample based on the following data to two decimal places- mass of beaker and cover: 50.09- mass of beaker, cover, and sample before heating: 51.04- mass of beaker, cover, and sample after heating: 50.88
Answers
Step 1 - Understanding the problem
We need to determine the mass of a sample which probably contains water as an impurity. Therefore, if we just weight the sample, we won't be able to separate its own weight from that of water.
What can be done, then, is heating the sample first in order to evaporate all the water, and only then weighting it. That's exactly what the procedure in the exercise has done.
The idea here thus is that we just need to subtract two weights:
[tex]m_{\text{sample}}=m_{\text{sample}+\text{water}}-m_{\text{water}}[/tex]Step 2 - Discovering the mass of the sample
We can discover the mass of the sample by simply subtracting the mass of beaker and cover from the final mass (beaker + cover + sample after heating).
This will give us the mass of the sample because the water has evaporated after heating:
[tex]m_{\text{sample}}=50.88-50.09=0.79g[/tex]The mass of the sample is thus 0.79g.
How must nuclear waste that is considered high-level waste to be stored
Answers
Answer: the best option to answer the question is the second one (letter B).
Explanation:
The question requires us to choose, among the options given, which one best corresponds to the correct form of disposal fo high-level nuclear waste.
High-level nuclear waste corresponds mainly to highly radioactive materials produced as byproducts of reactions that occur inside nuclear reactors. When they are not of use anymore, they are disposed in underground repositories, without any recycling. The place of disposal of this type of nuclear waste is usually placed in cannister which are placed underground and sealed with rocks. Since the time of decay of high-level nuclear waste can reach hundreds of thousands of years, this type of waste must be disposed of in a way that provides adequate protection for a long time.
Considering the information above, we can say that the best option to answer the question is the second one (letter B).
What are the OSHA PEL-TWyA and PEL-STEL values for nitric acid?
Answers
The OSHA limit for STEL-TWA is 2ppm and the PEL-STEL value is 4ppm to the exposure to nitric acid.
OSHA refers to Occupational Safety and Health Administration has adopted standard values for the exposure to harmful and hazardous chemicals so that the safety of workers and testing animals could be ensured.
Here, STEL-TWA stands for Short Term Exposure Limit - Time-Weighted average, and PEL-STEL stands for Permissible Exposure Limit- Short Term Exposure Limit.
This is usually set up in industries to ensure the safety of the workers and the maximum exposure short-term time limit is 15min and 2ppm for STEL-TWA and 4 ppm for PEL-STEL.
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you discover the head of a match contains 3.75 g of sulfur. How many atoms of sulfur does the match contain? (hint: grams > moles > atoms)
Answers
As the question says, we are going to follow the path of the hint, first by finding the number of moles of Sulfur in 3.75 grams, and we can do that by using its molar mass, which is 32g/mol
32g = 1 mol
3.75g = x moles
32x = 3.75
x = 3.75/32
x = 0.12 moles of Sulfur in 3.75 grams
Now we have the number of moles, and to find the number of atoms, we need to use the Avogadro's constant number, which is the number of atoms in a single mol, this value is 6.02*10^23 atoms in 1 mol
1 mol = 6.02*10^23 atoms
0.12 moles = x atoms
x = 7.22*10^22 atoms of Sulfur in 3.75 grams
4.68g of Si and 5.32g of O what is the mass percentage composition
Answers
According to the what was presented to me, to find the number of moles of a compound or element from a given mass, we need to use the molar mass of this element and do the following calculation:
Si = 28.0855g/mol
28.08g = 1 mol of Si
4.68g = x moles of Si
x = 0.17 moles of Si
O = 16g/mol
16g = 1 mol of O
5.32g = x moles of O
x = 0.33 moles of O
14) How many mL of 5.724 M HNO3 are needed to prepare a 183.95 mL of 2.063 M HNO3?
Answers
Answer
66.30 mL
Explanation
Given parameters:
Initial concentration, C₁ = 5.724 M
Final volume, V₂ = 183.95 mL
Final volume, V₂ = 183.95 mLFinal concentration, C₂ = 2.063 M
What to find:
The initial volume, V₁
Step-by-step solution:
Using the dilution law:
[tex]C_1V_1=C_2V_2[/tex]Substitute the given parameters into the formula to get V₁
[tex]\begin{gathered} 5.724M\times V_1=2.063M\times183.95mL \\ \text{Divide both sides by 5.724M} \\ \frac{5.724M\times V_1}{5.724M}=\frac{2.063M\times183.95mL}{5.724M} \\ V_1=66.30\text{ mL} \end{gathered}[/tex]Hence, 66.30 mL of 5.724 M HNO3 are needed to prepare a 183.95 mL of 2.063 M HNO3?
How many atoms (or molecules) are present in 1 mole?Question 19 options:A) 1B) 6.022×1020C) 6.022×1023D) 6.022
Answers
Answer:
The answer is C.
Explanation:
The number of particles (atoms/molecules) in 1 mole is referred to as the Avogadro's number. The Avogadro's number = 6.022 * 10 ^ 23. Therefore, the answer is C.
0.8g and 1.5g of two metals oxides were found countain 0.64g and 1.2g of metal respectively. show that this results obey law of definite proportion
Answers
Answer
This obey the law of definite proportion
Step-by-step explanation:
The Law of definite proportion states that any chemical compound will always contain a fixed ratio of elements by mass
According to the question,
Let the first oxide = x
Let the second oxide = y
x = 0.8g
y = 1.5g
For the first metal oxide, the amount of metal is 0.64 grams
Hence, the mass of oxygen is (0.8 - 0.64)
Mass of oxygen = 0.16g
Mass ratio = Mass of metal/mass of oxygen
Mass ratio = 0.64 / 0.16
Mass ratio = 4 : 1
For the second metal oxide, the amount of metal is 1.2g
Amount of oxygen = (1.5 - 1.2)
Mass of oxygen = 0.3
Mass of oxygen = 0.3g
Mass ratio = mass of metal/mass of oxygen
Mass ratio = 1.2 / 0.3
Mass ratio = 4: 1
Hence, the ratio of metals to oxygen is in the ratio of 4 to 1
Answer
Hence, this obey the law of definite proportion
What affect does a chemical reaction have on atoms?
Answers
Answer:Chemical reactions involve breaking chemical bonds between reactant molecules (particles) and forming new bonds between atoms in product particles (molecules).Explanation:
Is chlorine malleable or brittle?
Answers
Chlorine is not malleable or ductile. This is so because nonmetals, like chlorine, are brittle.
What is a chlorine physical characteristic?The odor of chlorine is distinctively intrusive and upsetting. The liquid is pure amber, while the gas is a greenish yellow tint. The information on the physical characteristics of chlorine as discovered by various researchers reveals some variances.
What is brittle versus ductile or malleable?In essence, metals that are malleable or ductile can both deform in some ways through plastic deformation in response to stress. Brittle metals are those that fracture without significant plastic deformation. Brittle is the antithesis of ductile and malleable in this context.
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Okay thanks so much I am watching it and watching
Answers
The twos are the subscript of each of element, those subscripts represent the number of atoms of each element that the molecule has. It means that the correct answer is Subscripts.
[OH﹘] = 6.5 x 10-5Mfind the pH and pOH
Answers
pH = 9.81
pOH = 4.19
Explanations:The formula for calculating the pOH of a solution is given as:
[tex]pOH=-log[OH^-][/tex]Given the following parameters
[tex][OH^-]=6.5\times10^{-5}M[/tex]Substitute
[tex]\begin{gathered} pOH=-log(6.5\times10^{-5}) \\ pOH=-(-4.19) \\ pOH=4.19 \end{gathered}[/tex]Determine the pH of the solution
[tex]\begin{gathered} pH+pOH=14 \\ pH=14-pOH \\ pH=14-4.19 \\ pH=9.81 \end{gathered}[/tex]Therefore the pH and pOH are 9.81 and 4.19 respectively
I need help getting the answer on all of theseFirst one
Answers
The Law of Conservation of Mass can be state in different ways. Essentially, this law states that if we are on a closed system, no mass can be created nor dstroyed. In chemical terms, this means that in a chemical reaction the number of atoms of each element has to be the same in the reactants and the products.
What is the coefficient of H2O in the balanced half reaction? (See picture)
Answers
Firstly we would determine the oxidation number of the elements to determine which is undergoing oxidation and which is undergoing reduction:
[tex]\begin{gathered} Mn\text{ }in\text{ }MnO_4^-:Mn+(-2\times4)=-1 \\ Mn\text{ }in\text{ }MnO_4^-:Mn-8=-1 \\ Mn\text{ }in\text{ }MnO_4^-:Mn=-1+8=+7 \\ \\ Mn\text{ }in\text{ }MnO_4^{2-}:Mn+(-2\times4)=-2 \\ Mn\text{ }in\text{ }MnO_4^{2-}:Mn=-2+8=+6 \end{gathered}[/tex]Mn oxidation number goes from +7 to +6 which means it is undergoing a reduction. A decrease in oxidation number means reduction.
[tex]\begin{gathered} S\text{ }in\text{ }HSO_3^-:1+(-2\times3)+S=-1 \\ S\text{ }in\text{ }HSO_3^-:1-6+S=-1 \\ S\text{ }in\text{ }HSO_3^-:S=-1+5=+4 \\ \\ S\text{ }in\text{ }SO_4^{2-}:S+(-2\times4)=-2 \\ S\text{ }in\text{ }SO_4^{2-}:S-8=-2 \\ S\text{ }in\text{ }SO_4^{2-}:S=+6 \end{gathered}[/tex]S oxidation goes from +4 to +6 meaning it is undergoing oxidation. There is an increase in oxidation number.
We will now balance the oxidation half reaction:
[tex]HSO_3^-+H_2O\rightarrow SO_4^{2-}+3H^++2e[/tex]The coefficient for the water molecule is 1 in the balnced half reaction.
How many grams of He gas are in a 33.2L container at 1.13atm and 652K?
Answers
Step 1
The He gas is assumed to be ideal. Therefore, the next equation is applied:
[tex]p\text{ x V = n x R x T \lparen1\rparen}[/tex]----------------------
Step 2
Information provided:
p = pressure = 1.13 atm
V = volume = 33.2 L
n = number of moles = unknown
T = absolute temperature = 652 K
R = gas constant = 0.082 atm L/mol K
---------------------
Step 3
Firstly, n is calculated from (1):
[tex]\begin{gathered} \frac{p\text{ x V}}{R\text{ x T}}=\text{ n} \\ \frac{1.13\text{ atm x 33.2 L}}{0.082\text{ }\frac{atm\text{ L}}{mol\text{ K}}x652\text{ K}}=0.702\text{ moles} \end{gathered}[/tex]n = 0.702 moles
----------------------
Step 4
The mass of He is calculated as:
n = mass/the molar mass He
The molar mass of He = 4.00 g
So, n = mass/4.00 g/mol
n x 4.00 g/mol = mass
0.702 moles x 4.00 g/mol = 2.81 g
Answer: mass = 2.81 g
You are creating a precipitate of silver chloride, starting with 1.00 mol of silver nitrate (AgNO3) and 0.75 mol of potassium chloride (KCl):AgNO3 (aq) + KCl (aq) → AgCl (s) + KNO3 (aq)What is the maximum amount of silver chloride (AgCl) that can be produced?Select one:a.0.75 molb.0.50 molc.1.00 mold.2.00 mol
Answers
Answer:
a. 0.75 mol
Explanation:
From the balanced equation, we know that 1 mole of AgNO3 reacts with 1 mole of KCl to produce 1 mole of AgCl and 1 mole of KNO3.
Since the ratio between AgNO3 and KCl is 1:1, in this case potassium chloride will be the limiting reactant and silver nitrate will be the excess reactant.
So we have to use the initial moles of the limiting reactant to calculate the moles of product that will be produced.
From the stoichiometry of the reaction we know that from 1 mole of KCl, we can obtain 1 mole of AgCl, so here the ratio between KCl and AgCl is also 1:1, so the maximum amount of silver chloride that can be produced is 0.75moles, as we can see using a mathematical rule of three:
[tex]\begin{gathered} 1molKCl-1moleAgCl \\ 0.75molesKCl-x=\frac{0.75molesKCl*1moleAgCl}{1molKCl} \\ x=0.75molesAgCl \end{gathered}[/tex]Calculate the percentage oxygen in dinitrogen pentoxide
Answers
So, To calculate the mass percentage of dinitrogen pentoxide (N2O5) we will first calculate the molar weight of the molecule. The mass percentage will be calculated with the following equation:
[tex]\text{Mass percentage = }\frac{\text{Molar Mass oxygen}}{MolarmassmoleculeN_2\text{O}_5}\times100[/tex]Molar mass will be:
Element Atomic Mass #Atoms Mass
N 14.0067 2 28.0134 g/mol
O 15.9994 5 79.997 g/mol
Total mass = 28.0134 + 79.997 = 108.0104 g/mol
[tex]\text{Mass percentage = }\frac{\text{7}9.997}{108.0104}\times100\text{ = }74.064\text{ percent}[/tex]Which statement is true about energy and bonds?A.Energy is absorbed when a bond forms.B.When bonds are formed, energy is released.C.A bond is formed as atoms are split apart from each other.D.Breaking bonds creates energy.
Answers
Answer
B. When bonds are formed, energy is released.
Explanation
The breaking of chemical bonds never releases energy to the external environment. However, energy is only released when chemical bonds are formed.
Therefore the only true statement about energy and bonds in the given options is:
B. When bonds are formed, energy is released.
Using the following chemical equation and your vast knowledge of stoichiometry, calculate the exact molarity of the NaOH. Hint—it should be around 0.1 M.KHP(aq) + NaOH(aq) NaKP(aq) + H2O(liquid)a)Convert the grams of KHP into moles of KHP using the formula weight of 204.2 grams per mole.b)Convert moles of KHP into moles of NaOH using the stoichiometry given in the above equation.c)Calculate the molar concentration of the NaOH by dividing the number of moles of NaOH calculated immediately above by the volume of NaOH used (measured using the buret). Be sure to convert the volume from mL to L.d)Average the three values obtained to determine the average molar the concentration of the NaOH. GET INFORMATION FROM THE PICTURE
Answers
ANSWER
The molar concentration of NaOH is 0.0705 mol/L
STEP-BY-STEP EXPLANATION:
Given the balanced equation below
[tex]\text{KHP}_{(aq)}+NaOH_{(aq)}\text{ }\rightarrow NaKP_{(aq)}+H_2O_{(l)}[/tex]According to the balanced equation, 1 mole of KHP gives 1 mole of NaOH
Given parameters
Molar mass of KHP = 204.2 grams/mol
To find the mole of KHP, we will need to find the average grams of KHP used
• For flask 1; 0.55g of KHP was used
,• For flask 2; 0.56g of KHP was used
,• For flask 3; 0.56g of KHP was used
The average mass of KHP used can be calculated below using the average formula
[tex]\begin{gathered} \text{Average mass = }\frac{mass\text{ 1 + mass 2 + mass 3}}{3} \\ \text{Average mass = }\frac{0.55\text{ + 0.56 + 0.56}}{3} \\ \text{Average mass = }\frac{1.166}{3} \\ \text{Average mass = 0.3886 grams} \end{gathered}[/tex]The average mass of KHP used is 0.3886grams
[tex]\begin{gathered} \text{Mole = }\frac{\text{ reacting mass}}{\text{molar mass}} \\ \text{reacting mass = 0}.3886\text{ grams} \\ \text{Molar mass = 2}04.2\text{ grams/mol} \\ \text{Mole = }\frac{0.3866\text{ }}{204.2} \\ \text{Mole of KHP = 0.0019 mole} \end{gathered}[/tex]The mole of KHP is 0.0019 mole
PART B
According to the balanced equation, the stoichiometry ratio of KHP to NaOH is 1: 1
Let the mole of NaOH be x
[tex]\begin{gathered} 1\text{ : 1 = }0.0019\text{ : x} \\ \frac{1}{1}\text{ = }\frac{0.0019}{x} \\ \text{Cross multiply} \\ 1\cdot\text{ x = 1 }\cdot\text{ 0.0019} \\ x\text{ = 0.0019 mole} \end{gathered}[/tex]Hence, the mole of NaOH is 0.0019 mole
PART C
Given the following parameters
0. The volume of NaOH used in flask 1 = 26.70mL
,1. The volume of NaOH used in flask 2= 27.09mL
,2. The volume of NaOH used in flask 3 = 26.96mL
The next step is to convert the mL to L
[tex]1mL\text{ = 0.001L}[/tex]For flask 1
[tex]\begin{gathered} 1mL\text{ = 0.001L} \\ \text{Let x be the volume of NaOH in L} \\ \text{ 1mL = 0.001L} \\ 26.70mL\text{ = xL} \\ \text{Cross multiply} \\ xL\cdot\text{ 1ml = 26.70mL }\cdot\text{ 0.001L} \\ x\text{ = }\frac{26.70\cdot\text{ 0.001}}{1} \\ x\text{ = 0.0267L} \end{gathered}[/tex]Using the same conversion process
The volume of NaOH in L in flask 2 = 0.02709L
The volume of NaOH in L in flask 3 = 0.02696L
Hence, the molar concentration of the solution in each flask can be calculated as follows
[tex]\text{Molar concentration = }\frac{concentration}{\text{Volume}}[/tex]For flask 1
Mole of NaOH = 0.0019 mole
Volume of NaOH = 0.0267L
[tex]\begin{gathered} \text{Molar concentration = }\frac{0.0019}{0.0267} \\ \text{Molar concentration = }0.0711\text{ mol/L} \end{gathered}[/tex]For flask 2
Mole = 0.0019 mole
Volume = 0.02709L
[tex]\begin{gathered} \text{Molar concentration = }\frac{Concentration}{\text{volume}} \\ \text{Molar concentration = }\frac{0.0019}{0.02709} \\ \text{Molar concentration = 0.0701 mol/L} \end{gathered}[/tex]For flask 3
Mole = 0.019mole
Volume = 0.02696 L
[tex]\begin{gathered} \text{Molar concentration = }\frac{concentration}{\text{volume}} \\ \text{Molar concentration = }\frac{0.0019}{0.02696} \\ \text{Molar concentration = 0.0704 mol/L} \end{gathered}[/tex]PART D
Average molar concentration can be found using the below formula
[tex]\begin{gathered} \text{Average molar concentration = }\frac{0.0711\text{ + 0.0701 + 0.0704}}{3} \\ \text{Average molar concentration =}\frac{0.2116}{3} \\ \text{Average molar concentraion = 0.0705 mol/L} \\ \text{The average molar concentration of NaOH is 0.0705 mol/L} \end{gathered}[/tex]What molarity of a 53.96 mL magnesium hydroxide solution is required to neutralize 93.24mL of a 7.306 M solution of hydrochloric acid solution, which creates as products, magnesium chloride and water?
Answers
Answer
6.312 M
Explanation
Given:
Volume of Mg(OH)₂, Vb = 53.96 mL
Volume of HCl, Va = 93.24 mL
Molarity of HCl, Ma =7.306 M
What to find:
The molarity of Mg(OH)₂, Mb
Solution:
The first step is to write a balanced chemical equation for the reaction.
Mg(OH)₂ + 2HCl → MgCl₂ + 2H₂O
Mole ratio is 1:2; that is na = 2 and nb = 1
Hence, the molarity of Mg(OH)₂, Mb is calculated using the formula below:
[tex]\frac{M_aV_a}{n_a}=\frac{M_bV_b}{n_b}[/tex]Plugging the values of the given parameters into the formula, we have:
[tex]\begin{gathered} \frac{7.306M\times93.24mL}{2}=\frac{M_b\times53.96mL}{1} \\ \\ Cross\text{ }multiply \\ \\ M_b\times53.96mL\times2=7.306M\times93.24mL\times1 \\ \\ Divide\text{ }both\text{ }sides\text{ }by\text{ }53.96mL\times2 \\ \\ \frac{M_b\times53.96mL\times2}{53.96mL\times2}=\frac{7.306M\times93.24mL\times1}{53.96mL\times2} \\ \\ M_b=6.312\text{ }M \end{gathered}[/tex]Therefore, the molarity of a 53.96 mL magnesium hydroxide solution that is required to neutralize 93.24mL of a 7.306 M solution of the hydrochloric acid solution is 6.312 M
A buffer solution is prepared by adding 275 mLof .676 M of HCI to 500 mL of .525M sodiumacetate. What is the pH of this buffer?
Answers
Explanation:
A buffer is a mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid. In our case we are reacting a strong acid (HCl) and a weak base (sodium acetate). So we don't have a buffer. The strong acid will neutralize the weak base. We have to determine which of them is in excess and find the pH of the resulting solution.
HCl (aq) + CH₃COONa (aq) ----> NaCl (aq) + CH₃COOH (aq)
First we have to determine the number of moles of each reactant. We added 275 ml of a 0.676 M solution of HCl and 500 mL of a 0.525 M solution of CH₃COONa. We can use the definition of molarity concentration to determine the number of moles of each reagent.
Molarity = moles of solute/volume of solution in L
moles of solute = molarity * volume of solution in L
moles of HCl = 0.676 M * 0.275 L
moles of HCl = 0.186 moles
moles of CH₃COONa = 0.525 M * 0.500 L
moles of CH₃COONa = 0.262 moles
HCl (aq) + CH₃COONa (aq) ----> NaCl (aq) + CH₃COOH (aq)
In the equation of the reaction all the coefficients are 1. So 1 mol of HCl will completely neutralize 1 mol of CH₃COONa. The molar ratio between them is 1 to 1.
1 mol of HCl = 1 mol of CH₃COONa
We mixed 0.262 moles of CH₃COONa with 0.186 moles of HCl. The 0.186 moles of HCl will neutralize 0.186 moles of CH₃COONa. And CH₃COONa will be excess.
Excess of CH₃COONa = 0.262 moles - 0.186 moles
Excess of CH₃COONa = 0.076 moles
Now we have to determine the concentration of this excess. We mixed 0.275 L with 0.500 L. Then the total volume of solution is 0.775 L. And the concentration of CH₃COONa after the reaction is:
total volume = 0.500 L + 0.275 L
total volume = 0.775 L
Resulting molarity of CH₃COONa = 0.076 moles/0.775 L
Resulting molarity of CH₃COONa = 0.098 M
Finally to get our answer we have to determine the pH of this resulting solution. To determine the pH of a weak base we have to use the ICE table. In solution
Answer:
What volume of O2 collected at 22.0 degrees Celsius and 728mmHg would be produced by the decomposition of 8.15g KClO3
Answers
The volume of O₂ collected at 22 degrees Celsius and 728 mmHg would be produced by the decomposition of 8.15 grams of KClO₃ is 2.52 L
It is given that the mass of KClO₃ is 8.15g and the temperature is 22°C and the pressure is 728mmHg. The number of moles of KClO₃ is given by,
No of moles of KClO₃ = 8.15/122.55
No of moles of KClO₃ = 0.066 mol
The reaction for decomposition is,
2KClO₃ -----------> 2KCl + 3O2
2 mol of KClO3 gives 3 moles of O₂
Then, 0.66mol of KClO3 gives, 3/2(0.66) mol of O₂ which is 0.0998
The given temperature is 22 + 273 = 295K
The given pressure is 728mmHg which is 728/760 which is 0.958 atm
We know that
PV = nRT
0.958 x V = 0.0998x 0.0821x295
V = 2.52L
Therefore, the volume of Oxygen collected is 2.52L
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Determine the mole fraction of NaCl in a solution that has 0.589 mol NaCl and 0.625 mol water.
Answers
Step 1
A mole fraction is defined as:
Mole fraction (compound X) = moles of compound X/total moles
It has no units
-------------------------
Step 2
The solution is formed by solute and solvent. Therefore, the total moles will be:
0.589 moles NaCl + 0.625 moles water = 1.214 moles
------------------------
Step 3
Molar fraction (NaCl) = moles NaCl/total moles = 0.589 moles/1.214 moles = 0.49 approx.
Answer: Molar fraction of NaCl = 0.49
17. What is a bond?
Answers
Bond:
Bonds are forces that keep atoms together to make compounds or molecules.
In chemical bonds electrons are involved. And there are three kinds of bonds:
1. Covalent bonds: where the electrons are shared between the atoms.
2. Polar covalent bonds
3. Ionic bonds: happens when one atom gives to the other atom electrons.
I have 2.50 x 10²³ atoms of titanium. How many moles of titanium do I have?
Answers
Answer: 2.50 x 10^23 atoms of titanium correspond to 0.415 moles of titanium.
Explanation:
The question requires us to calculate the number of moles of titanium (Ti) that correponds to 2.50 x 10^23 atoms of Ti.
We can apply the Avogadro's number to solve this problem: according to this proportionality constant, there are 6.022 x 10^23 particles in 1 mol of any compound (particles can be atoms, ions, molecules etc).
Thus, considering the Avogadro's number, we can write:
6.022 x 10^23 atoms Ti -------------------- 1 mol Ti
2.50 x 10^23 atoms Ti ---------------------- x
Solving for x, we'll have:
[tex]x=\frac{(1\text{ mol Ti\rparen}\times(2.50\times10^{23}\text{ atoms Ti\rparen}}{(6.022\times10^{23}\text{ atoms Ti\rparen}}=0.415\text{ mol Ti}[/tex]Therefore, 2.50 x 10^23 atoms of titanium correspond to 0.415 moles of titanium.
Which of the following ranks the molecules OF2, BF2, CF4, in order of their bond angles, from smallest to largest?
Answers
Answer:
[tex]\begin{gathered} BF_3:120\degree \\ CF_4:109.5\degree \\ OF_2:103\degree \\ OF_2Zinc metal reacts with HCl according to the balanced equation:Zn + 2HCl à ZnCl2 + H2When 0.103 g of Zn is combined with enough HCl to make 50 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.5 C to 23.7 C. Find the heat of the reaction. (ans: -160 kJ/mol)
Answers
-163kJ/mol
Explanations:Given the reaction between the zinc metal reacts with HCl according to the balanced equation:
[tex]Zn+2\text{HCl}\rightarrow\text{ZnCl}_2+H_2[/tex]The required heat of reaction will be calculated using the formula below:
[tex]\triangle H_{\text{rxn}}=-\frac{Q}{n_{Zn}}[/tex]where:
• Q is the ,heat produced
,• nZn is the, number of moles that reacted
The formula for calculating the quantity of heat produced is expressed as:
[tex]Q=mc\triangle\theta[/tex]where:
• m is the ,mass, of the ,Zinc metal
,• c is the ,specific heat capacity, of zinc
,• △θ is th,e change in temperature
Get the mass of zinc
[tex]\begin{gathered} \text{mass}=\text{ }density\times\text{volume} \\ m=\rho\times v \end{gathered}[/tex]The quantity of heat becomes:
[tex]Q=\rho\cdot v\cdot C\triangle\theta[/tex]Substitute the given parameters to have:
[tex]\begin{gathered} Q=\frac{1.02\cancel{g}}{\cancel{mL}}\times50\cancel{mL}\times\frac{4.18J}{\cancel{g^oC^{}}}\times(23.7-22.5)\cancel{^oC} \\ Q=1.02\times50\times4.18\times1.2 \\ Q=255.8Joules \end{gathered}[/tex]Next is to get the number of moles of Zinc that reacted (nZn)
[tex]\begin{gathered} nZ_n=\frac{Mass}{\text{Molar mass}} \\ nZ_n=\frac{0.103g}{65.4g\text{/mol}} \\ nZ_n=0.00157mole \end{gathered}[/tex]Get the required heat of reaction of Zinc:
[tex]\begin{gathered} \triangle H_{\text{rxn}}=-\frac{Q}{nZ_n} \\ \triangle H_{\text{rxn}}=-\frac{255.8Joules}{0.00157moles} \\ \triangle H_{\text{rxn}}=-162,929.93J\text{/mol} \\ \triangle H_{\text{rxn}}\approx-163kJ\text{/mol} \end{gathered}[/tex]Hence the heat of the reaction of Zinc is approximately -163kJ/mol