A 45.0 ml sample of nitric acid is neutralized by 119.4 ml of 0.2M NaOH. What is the molarity of the nitric acid?

The temperature required to obtain a final pressure of 675 mm Hg194 is .86 K.

An ideal gas is a theoretical gas composed of many randomly transferring factor particles that aren't difficult to interparticle interactions. the best gasoline idea is beneficial because it obeys the precise gas law, a simplified equation of country, and is amenable to evaluation under statistical mechanics.

Volume is a degree of occupied three-dimensional space. it's far more frequently quantified numerically the usage of SI-derived gadgets or by way of diverse imperial gadgets. The definition of length is interrelated with the extent.

An ideal gas is described as one for which both the extent of molecules and forces between the molecules are so small that they have got no effect at the behavior of the gas.

Using the ideal gas equation:-

Given;

P₁ =  549mm Hg =   0.722369 atm

V₁ = 8.5 L

T₁ = 268 K

P₂ =  675 mm Hg = 0.89 atm

V₂ = 5

T₂ = ?

P₁V₁/T₁ =P₂V₂/T₂

T₂ = P₂V₂T₁/P₁V₁

     = 0.89 × 5 ×  268 / 8.5  × 0.72

     = 194 .86 K

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Answer:

Explanation:

Here, we want to get another name for the theoretical value

The theoretical value is simply the value that has been accepted as true

Thus, we can call the theoretical value the true value

5 F2 (g) + 2 NH3 (g) → N2F4 (g) + 6 HF (g)

From the above balanced reaction, we can see that :

5 moles of F2 reacts to form : 6 moles of HF ,

so, 7.78moles F2 will give :x moles of HF

Therefore,x mole HF =( 6 moles HF * 7.78 mole F2)/ 5 mole F2

= 6 * 7.78/5

=9.336

≈9.34moles HF

• This means that , if you reacted 7.78 moles of F2 , ,9.34 moles of HF would be produced,.

Taking into account the Charles' Law, a sample of gas in a closed expandable container with an initial volume of 5.00 L was allowed to warm from 25°C to 35°C to a volume of 5.168 L.

Charles' Law consists of the relationship that exists between the volume and the temperature of a certain amount of ideal gas, which is maintained at a constant pressure.

This law says that for a given sum of gas at a constant pressure, as the temperature increases, the volume of the gas increases and as the temperature decreases, the volume of the gas decreases because the temperature is directly related to the energy of motion of the gas molecules.

In summary, Charles's law is a law that says that when the amount of gas and the pressure remain constant, the ratio between the volume and the temperature will always have the same value:

V÷T=k

Considering an initial state 1 and a final state 2, it is fulfilled:

V₁÷ T₁= V₂÷ T₂

In this case, you know:

Replacing in Charles' law:

5 L÷ 298 K= V₂÷ 308 K

Solving:

(5 L÷ 298 K)× 308 K= V₂

5.168 L= V₂

Finally, the new volume is 5.168 L.

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So,

The molecular mass of the empirical formula of the compound SO2, can be found multiplying the molar mass of each element by the number of atoms and then sum. Let me explain this here below:

We're given that the molecular mass of the molecular formula is 256g/mol. So, we could find the ratio between the mass of both formulas:

This means that the mass of the molecular formula is 4 times greater than the mass of the empirical formula.

Thus, the molecular formula will be:

Answer: Solubility

Explanation:

The property by which substances dissolve in water is called solubility. Soluble substances (such as salt) dissolve in water.

Answer: Electical charge

Explanation:At the molecular level, salt dissolves in water due to electrical charges and due to the fact that both water and salt compounds are polar, with positive and negative charges on opposite sides in the molecule.

Answer:

I am sure it's Transuranium.

Explanation:

Hope it's right

The final volume of the balloon if 0.20 moles of gas are added will be 1.62 L.

The volume of the balloon given that 0.20 moles of a gas is added to it is determined using the ideal gas equation as follows:

P₁V = nRT

Where;

Initial volume, V₁ = 1.50 L

Initial mole of gas, n₁ = 2.50 mol

Initial temperature, T₁= 25°C or 298 K

Initial pressure, P₁ = RT₁n₁/V₁

P₁ = 0.082 * 298 * 2.50 /1.50

P₁ = 40.7 atm

With pressure and temperature held constant:

Final temperature, T₂ is equal to T₁ = 298 K

Final pressure, P₂ is equal to P₁ = 40.7 atm

Final moles of gas, n₂ = 0.20 + 2.5

n₂ = 2.70 mol

Final volume, V₂ = RT₂n₂/P₂

V₂ =  0.082 * 298 * 2.70 /40.7

V₂ = 1.62 L

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MgSO4.7H2O

First of all, we need to calculate the molar mass of this molecule, using the periodic table.

Let's take each atomic mass of the elements that form this molecule from the periodic table.

Mg = 24.30 u

S = 32.06

O = 15.99 u

H = 1.007 u

Now, we have to do this:

Molar mass (g/mol) = 1 x 24.30 + 1 x 32.06 + 4 x 15.99 + 14 x 1.007 + 7 x 15.99

Molar mass = 246.3 g/mol

We have to be careful with this result because 246.3 g is the mass of 1 mole of MgSO4.7H2O and we want the mass of 1 formula unit or molecule.

Pay attention to this:

1 mole of MgSO4.7H2O = 246.3 g = 6.022 x 10^23 formula units or molecules of MgSO4.7H2O

(We want the mass of 1 molecule and we have just calculated the mass of 6.022x10^23 molecules)

----------------------------------------------------------------------------------------------------------------

For 1 formula unit or molecule:

246.3 g of MgSO4.7H2O ------------- 6.022 x 10^23 formula units or molec.

x ------------- 1 formula unit or molec.

Answer: The mass of 1 formula unit or molecule of MgSO4.7H2O = 4.09x10^-22 g

Answer:

Explanation:

Here, we want to get the temperature of the gas

We can use the ideal gas equation here

Mathematically, we have this as:

P is the pressure which is given as 34.56 kPa

V is the volume which is given as 440.99 mL

R is the molar gas constant which is 0.08205 L atm/mol k

n is the number of moles which is given as 1.43 mol

We need to convert the pressure to the correct unit (considering the molar gas consnat value in atm)

1 kPa = 0.00986923 atm

34.56 kPa will be = 34.56 * 0.00986923 = 0.341 atm

We need to convert the volume to Liters by dividing by 1000

We have that as 440.99/1000 = 0.44099 L

Finally,we rewrite the equation in terms of temperature and substitute the values as follows:

The molarity of a solution that contains 0.75 mol of KCI in 0.250L of the solution is 3 M

The number of moles per liter of solution is termed molarity.

M=n/V(in L)

M is the molarity

n is the number of moles

V is the volume

Substituting the values, we get

M=0.75/0.25=3

The molarity is 3 M

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Answer:

The charge of the metal is +5.

Explanation:

As the chlorine atom has a valence of -1, and the metals have a positive valence, we have to look for the charge that makes the molecule neutral.

In this case, there are 5 Cl, so the total negative charge of Cl is -5.

To make the molecule neutral, the metal must have a positive charge of +5.

Answer

2MnO₄⁻(aq) + 10Cl⁻(aq) + 16H⁺ → 2Mn²⁺(aq) + 5Cl₂(g) + 8H₂O

Explanation

What is given:

The following reaction takes place in an acidic solution:

MnO₄⁻(aq) + Cl⁻(aq) → Mn²⁺(aq) + Cl₂(g) (unbalanced).

What to find:

To identify the half-reactions and balance the redox reaction.

Step-by-step solution:

Step 1: Identify the half-reactions.

The oxidation half-reaction is: Cl⁻(aq) → Cl₂(g)

The reduction half-reaction is: MnO₄⁻(aq) → Mn²⁺(aq)

Step 2: Balance the equations for atoms (except O and H).

Oxidation: 2Cl⁻(aq) → Cl₂(g)

Reduction: MnO₄⁻(aq) → Mn²⁺(aq)

Step 3: Balance the equations for atoms O and H using H₂O and H⁺.

Oxidation: 2Cl⁻(aq) → Cl₂(g)

Reduction: MnO₄⁻(aq) + 8H⁺ → Mn²⁺(aq) + 4H₂O

Step 4: Balance the charge in the half-reactions.

Oxidation: 2Cl⁻(aq) → Cl₂(g) + 2e⁻

Reduction: MnO₄⁻(aq) + 8H⁺ + 5e⁻ → Mn²⁺(aq) + 4H₂O

Step 5: Multiply each half-reaction by the proper number to balance charges in the reaction.

Oxidation: 2Cl⁻(aq) → Cl₂(g) + 2e⁻ x 5

Reduction: MnO₄⁻(aq) + 8H⁺ + 5e⁻ → Mn²⁺(aq) + 4H₂O x 2

↓

Oxidation: 10Cl⁻(aq) → 5Cl₂(g) + 10e⁻

Reduction: 2MnO₄⁻(aq) + 16H⁺ + 10e⁻ → 2Mn²⁺(aq) + 8H₂O

Step 6: Add the equations and simplify to get a balanced equation.

2MnO₄⁻(aq) + 10Cl⁻(aq) + 16H⁺ + 10e⁻ → 2Mn²⁺(aq) + 5Cl₂(g) + 8H₂O + 10e⁻

Simplifying the equation, we have:

2MnO₄⁻(aq) + 10Cl⁻(aq) + 16H⁺ → 2Mn²⁺(aq) + 5Cl₂(g) + 8H₂O

Sulphur atom has 16 as its atomic number, which is also the same number of protons and the same number of electrons:

Z = 16

P = 16

e- = 16

But when we have a Sulphur ion, it is usually -2, and since we have 18 electrons in this case, the charge will be -2

• When Sodium Sulfate is mixed with Barium chloride, the following reaction occurs :

• a precipitate is the solid that forms, the white solide will be BaSO4

• So option 4 is correct. BaSo4.

In order to solve this question, we can use the concept of molar ratio, which means the amount of reactant is needed in order to produce a certain amount of product. In our question we have:

2 C2H2 + 5 O2 -> 4 CO2 + 2 H2O

The molar ratio between O2 and H2O is 5:2 (we use only the numbers in front of the compound), so that means that for every 5 moles of O2 used, we will have 2 moles of H2O being produce, now we can use this information to calculate how many moles of H2O will be produced from 3.80 moles of O2

5 O2 = 2 H2O

3.80 O2 = x H2O

x = 1.52 moles of H2O are produced from 3.80 moles of O2

The formulas and and  the names for 5 possible ionic compounds involving these ions are :

Rb₂O, Rubidium Oxide

FeCl₂, Iron(II)chloride

Al(OH)₃ , Aluminum hydroxide

LiH, Lithium Hydride

NaCl, Sodium chloride

1) The  Rb₂O is called as Rubidium oxide. rubidium oxide is an ionic compound. Ionic compound formed between a positive ion called cation and a negative ion called anion . ionic bond is formed with the complete transfer of electrons. In Rubidium oxide : the cation is Rb⁺ and the anion is O²⁻.

2) The FeCl₂ is called as iron(II)chloride. iron(II)chloride is an ionic compound. in  iron(II)chloride : the cation is Fe²⁺ and the anion is Cl⁻.

3) Al(OH)₃ is aluminum hydroxide . In aluminum hydroxide : the cation is present as Al³⁺ and anion is present as OH⁻.

4) LiH is lithium hydride . the cation is Li⁺ and the anion is H⁻.

5) NaCl is sodium chloride. cation is Na⁺ and anion is Cl⁻

Thus, The formulas and and  the names for 5 possible ionic compounds involving these ions. Rb₂O, Rubidium Oxide

FeCl₂, Iron(II)chloride

Al(OH)₃ , Aluminum hydroxide

LiH, Lithium Hydride

NaCl, Sodium chloride

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-292.8J/mmol

Given the reaction of NaCl and NaOH expressed by the chemical equation:

Amount of heat released when one mole of strong acid reacts with one mole of the strong base is -48.8 kJ/mmol.

If 6 moles of the sample acid reacts with 6 moles of NaOH, the required enthalpy cheange is expressed as:

Hence the enthalpy change if you neutralized six moles of HCl with an equal number of moles NaOH is -292.8J/mmol

Answer:

Explanation:

Here, we want to get the number of moles in 2.24 L of a sample of gas

Mathematically,

At STP, 1 mole of a gas occupies a volume of 22.4 L

Thus x moles will occupy 2.24 L at STP

To get the value of x, we have it that:

Answer: Joules (J)

Explanation:

Answer:

Joules or Newton metre

Explanation:

Work = Force × distance

Force = kgm/s² (Newton)

×

Distance = m

= kgm²/s² (Newton metre or Joules) (Nm or J)

Answer

The mole ratio of H2O to H2SO4 is 2:1

Explanation

Given chemical equation:

From the balanced chemical equation above, 2 moles of NaOH react with sulfuric acid, 1 mole of H2SO4, to produce 2 moles of water and 1 mole sodium sulfate.

So, from the chemical equation, you have a 2:1 mole ratio between H2O and H2SO4

Answer

• Carbon has the atomic symbol C,

• Carbon is a nonmetallic chemical element with 4 electrons in its valence shell, which allows it to form 4 bonds forming compounds like CH₄.

• Reactivity: Carbon does not dissolve in or react with water or acids.

• The atomic mass of carbon is 12.011 g. It contains 6 protons in its nucleus.

Remember that standard temperature and pressure (STP) is when the pressure is 1 atm and the temperature is 0 °C (273 K).

The answer is 273 K and 1 atm.

In order to find the number of moles in a given mass of any compound, we need to use the molar mass of this compound, which is the total mass present in 1 mol of the compound. The molar mass of CaSO4 is 136.14g/mol

136.14 grams = 1 mol of CaSO4

37.16 grams = x moles of CaSO4

136.14x = 37.16

x = 37.16/136.14

x = 0.27 moles of CaSO4

In 37.16 grams, we will have 0.27 moles of CaSO4

Answer

4.94x10^22 molecules

explanation

to calculate the number of molecules in 8.21x10^-2 moles ca be determined by using Avogadros number

we know that

1 mol has 6.022x10^23 molecules

therefore,

8.21x10^-2 moles have:

(8.21x10^-2) x (6.022x10^23)

= 4.94x10^22 molecules

Step 1 - Understanding how mole relates to temperature, pressure and volume

These variables are related according to the ideal gas equation:

We can use this equation to predict the behavior as well as the quantity of a gas, given that the remaining variables are given.

Step 2 - Using the equation to solve the equation

According to the exercise:

Setting the values in the equation:

We need to make two observations now: the temperature must be in Kelvin in this equation for it to work. R stands for the universal gas constant, as has the value of 0.082 atm.L/mol.K.

Therefore:

Answer: the amount of moles used is 0.17 moles.

Answer: the best option to answer the question is letter A

Explanation:

The question requires us to choose the option that presents the formula of two alkanes.

Alkanes are hydrocarbons that are saturated and acyclic (i.e., the molecule of an alkane do not present double or triple bonds between carbons and it is a linear structure). The general formula of alkanes tells us that there are double plus 2 the amount of hydrogen atoms as there is carbon atoms, as it follows:

where n indicates the number of carbon atoms in the molecule.

For example: we can say that the compound C2H6 is an alkane because it contains 2 carbon atoms (n = 2) and 6 hydrogen atoms (2n +2= 6).

Considering the options given by the question, only option A presents the formula of two alkanes:

CH4: n = 1; 2n+2 = 2+2 = 4

C8H18: n = 8; 2n+2 = 16+2 = 18

Therefore, the best option to answer the question is letter A.

Answer

47.60 g

Explanation

Given that:

Molar mass of MgCl₂ = 95.20 g/mol

Mass of Mg produced = 12.15 grams

Equation: MgCl₂ → Mg + Cl₂

What to find:

To calculate the grams of MgCl₂ needed to produce 12.15 grams of Mg.

Step-by-step solution:

Step 1: Convert the mass of Mg produced to moles.

Using the molar mass of Mg (24.305 g/mol) and the mole formula, the moles of Mg produced is

Step 2: Determine the moles of MgCl₂ needed to produce 12.15 g of Mg.

According to the given equation; 1 mol of MgCl₂ produced 1 mol of Mg

So, x mol of MgCl₂ will produce 0.49989714 mol of Mg

That is:

Step 3: Convert the moles of MgCl₂ needed to produce 12.15 g of Mg to grams.

Using the molar mass of MgCl₂ = 95.20 g/mol, therefore the mass in grams of MgCl₂ needed to produce 12.15 g of Mg will be:

Hence, the grams of MgCl₂ needed to produce 12.15 grams of Mg is 47.60 g.

CH3CH3

CH3SCH3

CH3CH2OH 

What are organic compounds?

Organic compounds are compounds that class of compounds that contains the carbon-hydrogen bond. This means that for a compound to be classified as an organic compound, they must contain the C-H bond in their compound

From the listed compouds, the compound that contains theC-H bonds are:

• CH3CH3

• CH3SCH3

• CH3CH2OH

These are therefore considered the required list of organic compounds from the given options