Answer:
[tex]2\text{ : 2 single bonds to carbon and 1 double bond to a carbon}[/tex]Explanation:
Here, we want to describe the correct Lewis diagram for the molecule
For the molecule, we will have a double bond between the two central carbon atoms. Then, we will have 2 single bonds from each carbon atom to the hydrogen atoms.
Thus, the correct answer choice here is 2 single bonds to carbon and 1 double bond to a carbon
The correctly drawn Lewis structure for CH₂CH₂ will have 2 single bonds to carbon and one double bond to carbon. Therefore, the correct option is option 2.
A Lewis structure is a representation of a molecule or ion that shows the arrangement of atoms, the bonding between them, and the distribution of valence electrons. It is a simplified way to visualize the electronic structure of a compound.
In a Lewis structure, atoms are represented by their chemical symbols, and valence electrons are represented as dots or lines. Dots are placed around the atomic symbols to indicate non-bonding electrons, and lines represent covalent bonds between atoms. Lewis structures help in understanding the bonding and molecular geometry of a compound, as well as predicting its chemical behavior.
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It took 13,750 Joules of energy to raise the temperature of water to 45.0 °C. If you have 125.0 grams
of water and the specific heat of water is 4.18 J/g °C, what is the starting temperature?
The initial temperature of water can be calculated from the heat energy using calorimetric equation. The initial temperature is obtained as 18.65 °C.
What is calorimetric equation?Calorimetry is an analytical tool used to determine the heat energy absorbed or released in a chemical reaction. The heat energy q, mass of the substance m and the specific heat capacity c with a temperature difference ΔT is written as follows:
q = m c ΔT.
Here, the heat energy required for raising the temparture of 125 g of waater to 45 °C is 13750 joules . Then, the initial temperature be x, then x can be calculated as follows:
13750 J = 125 g × 4.18 J/g °C × (45 - x °C)
x = 45 - [ 13750 J / (125 g × 4.18 J/g °C) ]
= 18. 65 °C.
Therefore, the initial temperature was 18. 65 °C.
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How many grams of H2O are in 0.2 moles of H2O (molar mass 18.01 g/mol)?
The number of grams in 0.2 moles of water is 3.602grams.
How to calculate mass?The mass of a substance can be calculated by multiplying the number of moles of the substance by its molar mass as follows:
Mass = molar mass × no. of moles
According to this question, there are 0.2 moles in water. Water has a molar mass of 18.01g/mol. The mass can be calculated as follows:
Mass = 0.2 moles × 18.01g/mol
Mass = 3.602grams.
Therefore, 3.602 grams is the mass of the water molecule.
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Sodium reacts with oxygen to produce sodium oxide.4Na(s)+O2(g)→2Na2O(s)If you have 16.0 g of Na , how many grams of O2 are required for the reaction?
5.57 grams
Explanations:Given the reaction between sodium and oxygen expressed as:
[tex]4Na(s)+O_2(g)\rightarrow2Na_2O(s)[/tex]Given the following parameters
Mass of sodium = 16.0g
Determine the moles of sodium
[tex]\begin{gathered} moles\text{ of Na}=\frac{mass}{molar\text{ mass}} \\ moles\text{ of Na}=\frac{16}{23} \\ moles\text{ of Na}=0.6957moles \end{gathered}[/tex]According to stoichiometry, 4 moles of sodium reacts with 1 mole of oxygen, the moles of oxygen that reacted is given as;
[tex]\begin{gathered} moles\text{ of O}_2=\frac{0.6957}{4} \\ moles\text{ of O}_2=0.1739moles \end{gathered}[/tex]Determine the mass of oxygen that reacted
[tex]\begin{gathered} mass\text{ of O}_2=mole\times molar\text{ mass} \\ mass\text{ of O}_2=0.1739\times32 \\ mass\text{ of O}_2=5.57grams \end{gathered}[/tex]Hence the mass of oxygen that reacted is 5.57 grams
1) Write the equation for the reaction used to generate oxygen gas. Word Equation: Formula Equation:
For the generation of oxygen gas, hydrogen peroxide is generally used and by means of a catalyst, the peroxide is decomposed into two compounds: Liquid water and oxygen gas. The reaction is as follows:
Word equation
Hydrogen peroxide --->Water + Oxygen
Formula equation
[tex]2H_2O_2(aq)\rightarrow^{}2H_2(l)+O_2(g)[/tex]It is important to note that the reaction needs a catalyst.
(b) Determine the kilocalories needed to heat 2.55 kg water from 21 °C to 37 °C.
Calculations:
We are given the following parameters :
• Mass = 2.55kg = 2.55*1000= 2550
,• T1 = 21°C
,• T2 = 37°C
,• Specific heat of water = c = 1cal/g°C
We will calculate q (heat ) as follows :
[tex]\begin{gathered} Q\text{ = m }\cdot c\cdot\Delta T \\ \text{ = 255}0\cdot\text{ }1\cdot\text{ ( 37-21)} \\ \text{ =}2550\cdot\text{ 16} \\ \text{ = 40800 calories }\ldots\ldots(\text{divide by 1000 to get to kilicalories) } \\ \text{ =40.8 kilocalories } \end{gathered}[/tex]A nurse practitioner prepares an injection of promethazine, an antihistamine used to treat allergic rhinitis. If the stock bottle is labeled 25 mg/mL and theorder is a dose of 15.0 mg, how many milliliters will the nurse draw up the syringe? Express the volume in milliliters to two significant figures.
Explanation:
We are given: density of promethazine = 25mg/mL
: mass of promethazine = 15.0mg
[tex]\begin{gathered} D\text{ = }\frac{m}{V} \\ \\ \therefore V\text{ = }\frac{m}{D} \\ \\ \text{ = }\frac{15}{25} \\ \\ \text{ = 0.60 mL} \end{gathered}[/tex]Answer:
The nurse will draw up 0.60 mL.
Ksp= 2×10−19 for LaF3 Calculate the solubility of LaF3 in grams per liter in a solution that is 0.055 M in LaCl3
First, we write our reaction:
We call solubility to "S"
LaF₃(s) → La³⁺(aq) + 3 F⁻(aq)
Initial - 0.055M (LaCl3) 0
Change +S +3.S
Eq. 0.055+S 3.S
Ksp = 2×10^−19 = [La³⁺]x[F⁻]³ = (0.055+S)x(3.S)³
2×10^−19 = (0.055+S)x(3.S)³ => S = 5.12x10^-7 mol/L x (195.9 g/mol) =>
S = 1.00x10^-4 g/L
(195.9 g/mol = The molar mass of LaF3)
Answer: S = 1.00x10^-4 g/L
Pls help me I don’t know how to do this asap help
Answer:
[tex]17.65\text{ \%}[/tex]Explanation:
Here, we want to get the percentage by mass of the water molecules in the given compound
To get this, we have to divide the molar mass of water by the molar mass of the percentage and write the answer as a percentage
The molar mass of water is 18 g/mol
The molar mass of MgCO3 is 84 g/mol
Thus, the percentage by mass of water will be:
[tex]\frac{18}{18\text{ + 84}}\text{ }\times\text{ 100 \% = 17.65 \%}[/tex]Which element ,cesium or francium easily loses electron ? Justify your answer in terms of atomic size and attraction towards the positive nucleus
Francium easily loses electrons than cesium
Explanations:Both Cesium and Francium are Group 1 elements (Alkali metals). This shows that the elements in this group have one valence electron in their outermost shell and can easily lose this electron to form a stable atom.
According to the element in the group, Lithium has the least tendency to loose its valence electron while Francium has the highest tendency to lose its valence electron because its outermost electron gets further from the positive nucleus and less attracted by the nucleus compared to the Caesium element.
Also, the atomic size of Francium is greater than that of Caesium. This also shows that francium easily loses electrons than cesium
Assign oxidation numbers to each atom in the following compounds or ions: a. HFb. C/4c. H₂0d. Pl3e. CS₂f. Na₂O₂g.H₂CO3h. NO 2i. SO2-4Deforming the oxidation numbers for iron oxide Fe-On (Recall that oxidation numbers are integers)
Some oxidation number rules
1) The oxidation number of a free element is always 0. The atoms in He and N2, for example, have oxidation numbers of 0.
2) The usual oxidation number of hydrogen is +1.
3 The oxidation number of oxygen in compounds is usually -2. Exceptions include OF2 because F is more electronegative than O, and BaO2, due to the structure of the peroxide ion, which is [O-O]2-.
a) HF, H = +1 F = -1
b)
c) H₂0, H = +1 O = -2
d) Pl3, P = +3 I = -1
e) CS₂, C = +4 S = -2
f) Na₂O₂, Na = +1 O = -1
g) H₂CO3 H = +1 C =+4 O =-2
h) NO2 N = +2 O = -2
i) SO2-4 S =+6 O = -2
Name the following ester molecule:OA. ethyl butanoateB. propyl pentanoateC. methyl heptanoateD. methylpropanoate
Answer
A. ethyl butanoate
Explanation:
Esters are known for their distinctive odors and are commonly used for food aroma and fragrances. The general formula of an ester is RCOOR'.
Esters are formed through reactions between an acid and an alcohol with the elimination of water.
Esters are named as if the alkyl chain from the alcohol is a substituent. No number is assigned to this alkyl chain. This is followed by the name of the parent chain from the carboxylic acid part of the ester with an –e remove and replaced with the ending –oate.
Hence, the name of the given ester is:
A. ethyl butanoate
The most prominent line in the spectrum of magnesium is 285.2 nm. Other lines are found at 383.8 and 518.4 nm.
What is the energy of 1 photon of the light with the wavelength of the most energetic line?
The energy of the 1 photon of the light with the wavelength of the most energetic line is 6.9 * 10^-19 J.
What is the energy of a photon?We know that a photon can only be explained as simply as possible as a bundle of light. The photon is emitted from an atom when an electron in the atom is seen to move from a higher to a lower energy level thereby emitting light of the appropriate wavelength.
Now we can see that the wavelength that is the shortest is the one that would have the greatest energy. This is because the energy of the photon is inversely proportional to the energy of the photon.
Now we have';
Wavelength of the photon = 285.2 nm or 285.2 * 10^-9 m
Speed of light = 3 * 10^8 m/s
Plank's constant = 6.6 * 10^-34 J/s
Then;
E = 6.6 * 10^-34 J/s * 3 * 10^8 m/s/ 285.2 * 10^-9 m
E = 6.9 * 10^-19 J
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What is the energy of a photon of light that has a frequency of 7.87 × 10^15 Hz?
The question requires us to calculate the energy of a photon given that its frequency is 7.87 × 10^15 Hz.
To calculate the energy of a photon, we can use the following equation:
[tex]E=h\times f[/tex]where h is the Planck's constant (6.626 x 10^-34 Jxs) and f is the frequency (in Hz or 1/s). (Note that the unit Hz is equivalent to s^-1)
Then, applying the frequency provided and the Planck's constant to the equation, we have:
[tex]E=(6.626\times10^{-34}J\mathrm{}s)\times(7.87\times10^{15}s^{-1})=5.21\times10^{-18}J[/tex]Therefore, the energy of the photon is 5.21 x 10^-18 J.
Which of the following can be observed without changing the identity of a substance? Select all that apply.Boiling pointFlammabilityDensityReactivity
1) Boiling point - It is easy to observe the boiling point of a substance because it is only a physical process, raising the temperature enough to get to its boiling point.
2) Flammability - Observing the flammability of a substance has the effect of decomposing the substance because of the combustion, therefore its identity is not preserved.
3) Density - We can observe the density of a substance without changing its identity since it is just the relation between mass and volume.
Reactivity - The way to observe the reactivity of a substance is by undergoing a reaction with it, resulting in products that differ from the initial substance, so it is not possible to observe reactivity without a change in the substance.
Final answer: Boiling point and density can be observed without a change in the identity of a substance
What is the following of element P and P^3- :Orbital DiagramLong NotationShort NotationValence LevelGroup on Periodic TablePeriod on Periodic Table
We are asked to find some characteristics of phosphorus. We start with the yu period group to which they belong in the periodic table. This information is found in the periodic table of elements.
Looking in the periodic table we find that phosphorus P is located in group VA (15) and in period 3.
The electronic configuration depends on the number of electrons of the element. Phosphorous has 15 electrons. We have an ion P^3-, this ion has three more electrons, so for this element, we will have 18 electrons. The electronic configuration will be:
The short notation depends of another element, in this case of Ne, so the shot notation will be:
[tex]\lbrack Ne\rbrack3s^23p^6[/tex]The valence level is the last energy level, we see that the greatest coefficient is 3, so the valence level is 3
In summary, we have that the answer will be:
Orbital Diagram: Drawn in the picture
Long Notation: 1s2 2s2 2p6 3s2 3p6
Short Notation: [Ne] 3s2 3p6
Valence Level: 3
Group on Periodic Table: 15 or VA
Period on Periodic Table: 3
Please help solve What is the molarity of a solution that has 2.5 mol of NaOH dissolved in 10.0 L of H2O?
ANSWER
The molarity of the solution is 0.25M
EXPLANATION
Given that;
The mole of NaOH is 2.5 mol
The volume of the solution is 10.0L
Follow the steps below to find the molarity of the solution
The molarity formula is given below as
[tex]\begin{gathered} \text{ Molarity = }\frac{\text{ number of moles }}{\text{ volume of solution}} \\ \end{gathered}[/tex]Substitute the given data into the above formula
[tex]\begin{gathered} \text{ Molarity = }\frac{\text{ 2.5 }}{\text{ 10.0}} \\ \text{ Molarity = 0.25 M} \end{gathered}[/tex]Therefore, the molarity of the solution is 0.25M
A volume of 56.0 mL of He at STP. a. How much weight? b. How many molecules?
Answer
Number of moles = 0.0025 mol
Step-by-step explanation:
Given that,
The volume of He at STP is 56.0 ml
Part a:
Find the mole
According to the standard conversion
1 mol = 22.4L
Firstly, we need to convert 56.0ml to L
This can be done by dividing by 1000
56.0mL = 0.056L
1 mole = 22.4L
x mole = 0.056L
Cross multiply
1 * 0.056 = x * 22.4
0.056 = 22.4x
Divide both sides by 22.4
x = 0.056 / 22.4
x = 0.0025 mole
Hence, the mole of Helium is 0.0025 moleHe
Ethanol, C,H,O, is added to gasoline to produce "gasohol,"a fuel for automobile engines. How many grams of O₂ arerequired for complete combustion of 421 g of ethanol?2CO₂(g) + 3H₂O(g)C₂H₂OH()+ 30₂(g)Ethanol
We have the ethanol combustion reaction to produce CO2 and water. The balanced equation of the reaction is:
[tex]4C_2H_2OH+9O_2\rightarrow8CO_2+6H_2O[/tex]We must first find the moles of ethanol corresponding to 421 grams. To do this we divide the mass by the molar mass of ethanol. The molar mass of ethanol is: 46.07g/mol. The moles of ethanol will be:
[tex]molC_2H_2O=421gC_2H_2O\times\frac{1molC_2H_2O}{46.07gC_2H_2O}=9.14molC_2H_2O[/tex]Now, by the stoichiometry of the reaction, we see that the Oxygen to Ethanol ratio is 9/4. So, the moles of oxygen needed will be:
[tex]molO_2=9.14molC_2H_2O\times\frac{9molO_2}{4molC_2H_2O}=20.6molO_2[/tex]We find the grams of oxygen by multiplying the moles by the molar mass. The molar mass of O2 is 31.9988g/mol.
[tex]gO_2=20.6molO_2\times\frac{31.9988gO_2}{1molO_2}=658gO_2[/tex]Answer: To complete the combustion of 421 g of ethanol are needed 658 grams of oxygen
This is the question I need help with. I would really love to understand how reduction occurs here. Thanks in advance for helping me understand this.Which option describes a situation in which reduction occurs?Cl2 becoming Cl–Cl, 2, becoming Cl, –Xe2+ becoming Xe6+Xe, 2+, becoming Xe, 6+Al becoming Al3+Al becoming Al, 3+S2– becoming S
In chemistry, reduction means any of a class of chemical reactions in which the number of electrons associated with an atom or a group of atoms is increased.
You can say that a compound that is gaining electrons is being reduced.
The situation where the reduction is occurring is:
[tex]Cl^2\to Cl^-,[/tex]When the reduction occurs, the oxidation number (which is the superindex), it seems that is reducing this number. In this case, 2+ become 1-.
Remember: when the oxidation number is reducing, it means that the compound or element is a reduction (gaining electrons) and when the oxidation number is increasing, it means that it is oxidation (losing electrons) such as the other cases of the problem.
I need help on number 1 please
Answer:
Atom 1 and Atom 4 of the elements below are in the same group in the periodic table.
What is the total number of moles of products formed when 1.20 moles of ammonia reacts? 4NH3+5O2 --> 4NO+6H2O
Explanation:
Step 1 - We need to rewrite the equation here:
4NH3+5O2 --> 4NO+6H2O
The ratio between ammonia (NH3) and the products are:
NH3 and NO:
4:4
NH3 and H2O:
6 H2O
So if we have 1.2 moles of ammonia:
1.2 moles of NH3 ---- x moles of NO
4 moles of NH3 ---- 4 moles of NO
x = 1.2 moles of NO
1.2 moles of NH3 --- x moles of H2O
4 moles of NH3 --- 6 moles of H2O
4x = 7.2
x = 7.2/4
x = 1.8 moles of H2O.
Answer: The total number of moles of products formed is 1.2 moles of NO and 1.8 moles of H2O.
can anyone help me with this question
6.5 moles of gas will fill 1.7 litres at 1.3 atm at the temperature (in K). 546atmK273K=P, and 1atm273K = P.
How would you define temperature?Temperature is a measurement used to represent hotness and coolness on any of a number of scales, including Fahrenheit or Celsius. According to temperature, heat energy will naturally move from a hotter (body with a high temp) to a cooler (body with such a lower temperature) (one at a lower temperature).
What portion of your body is the hottest?The scrotum is the area of the body with the highest temperature (37°C), following by the ears, urine, as well as the mouth. The coldest temperature on human body that can usually be measured is the armpit (35.9°C).
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If gas has a pressure of 954 atm and temp of 728 k and the temp changes to 951 k what is the new pressure ?
We have a change of pressure and temperature. To solve and find the new pressure we will assume that the volume and moles of the gas remain constant, therefore we can apply Gay-Lussac's law which tells us:
[tex]\frac{P_1}{T_1}=\frac{P_2}{T_2}[/tex]Where,
P1 is the initial pressure of the gas, 954atm
T1 is the temperature of the gas, 728K
T2 is the final temperature, 951K
P2 is the final pressure, =?
We clear P2 and replace the known data:
[tex]\begin{gathered} P_2=\frac{P_1}{T_1}\times T_2 \\ P_2=\frac{954atm}{728K}\times951K=1246atm \end{gathered}[/tex]Answer: The new pressure will be 1246atm
Discribe a dehydration reaction?
The question requires us to describe a dehydration reaction.
In chemistry, a dehydration reaction is defined as a chemical reaction that involes the loss of water from the reactant. In other words, a dehydration reaction happens when the water molecule is formed from the one (or two combined) reactant.
Calculate the mass percent by volume of 44.1 g of glucose (C₆H₁₂O₆, MM = 180.2 g/mol) in 325 mL of solution.
13.1% m/v is the mass percent by volume of 44.1 g of glucose (C₆H₁₂O₆, MM = 180.2 g/mol) in 325 mL of solution.
[tex]% m/v=mass solute/volume solution * 100%=42.6g/325mL *100%=13.1%m//v[/tex]% m/v = mass solute/volume solution x 100%
[tex]% m/v=mass solute/volume solution * 100%=42.6g/325mL *100%=13.1%m//v[/tex]% m/v =44.1g/325 mL x 100%
[tex]% m/v=mass solute/volume solution * 100%=42.6g/325mL *100%=13.1%m//v[/tex]% m/v =13.1% m/v
An object's volume in three dimensions is determined by the area encompassed inside its boundaries. It is also known as the object's capability on occasion. Calculating how much is required to fill an object can be done using its volume; for example, how much water is required to fill a bottle, aquarium, or water tank.
The most fundamental and typical kind of three-dimensional form is a sphere. Spheres are frequently seen as balls, globes, holiday lights, oranges, etc.
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NH3 + O2 → ___NO2 + _H2O
Answer
Explanation
Given unbalanced equation:
NH₃ + O₂ → ___NO₂ + _H₂O
Step 1: Balance the N atom on both sides by putting 4 as the coefficient of NH₃ and NO₂ on the reactant and product sides of the equation respectively.
4 NH₃ + O₂ → 4 NO₂ + _H₂O
Step 2: Balance the H atom on both sides by putting 4 as the coefficient of NH₃ and NO₂ on the reactant and product sides of the equation respectively.
For the following reaction, how many grams of H2O will be produced if you react 3.7 grams of B2H6?B2H6 + 3 O2 → 2 HBO2 + 2 H2O
From the chemical equation we see that 1 mole of diborane (B2H6) will produce 2 moles of water.
We will firstly calculate the moles of diborane:
[tex]\begin{gathered} _nB_2H_6=\frac{mass}{molar\text{ }mass} \\ \\ _nB_2H_6=\frac{3.7g}{27.7\text{ }gmol^{-1}} \\ _nB_2H_6=0.134\text{ }moles \end{gathered}[/tex]One mole of diborane produces 2 moles of water then to find the moles of water that is produced we:
[tex]\begin{gathered} _nH_2O=2\times0.134\text{ }mole \\ _nH_2O=0.268 \end{gathered}[/tex]We then convert the moles of the water to mass:
[tex]\begin{gathered} mass=moles\times molar\text{ }mass\text{ }H_2O_ \\ \\ mass=0.268\text{ }mol\times18\text{ }gmol^{-1} \\ \\ mass=4.824g \end{gathered}[/tex]Mass of water is 4.824g
What is the limiting reactant if 2.50 moles of zinc react with 1.00 mole of sulfur? Zn + S—-> ZnS
Step 1
The reaction provided:
Zn + S => ZnS (completed and balanced)
-------------------
Step 2
Information provided:
2.50 moles of Zn
1.00 mole of S
--------------------
Step 3
The limiting reactant limits the amount of product formed.
By stoichiometry, procedure:
Zn + S => ZnS
1 mole Zn ------------- 1 mole S
2.50 moles Zn -------------- X
X = 2.50 moles Zn x 1 mole S/1 mole Zn = 2.50 moles S
For 2.50 moles of Zn, 2.50 moles of S are needed but there is only 1.00 mole of S. Therefore, the limiting reactant is S.
Answer: Sulfur (S)
Experiments were done on a certain pure substance X to determine some of its properties. There's a description of each experiment in the table below.In each case, decide whether the property measured was a chemical or physical property of X, if you can. If you don't have enough information to decide, choose can't decide in the third column.QA sample of solid X is carefully weighed and put inside a sealed flask. Pure hydrogen gas is added to the flask, and the mixture heated until the hydrogen starts being consumed. After hydrogen stops being consumed, the contents of the flask are removed and weighed, and from the increase in weight the value of may be calculated.physicalchemical(can't decide)MA small sample of X is put on the pan of a sensitive balance and its weight measured. Next, a magnet is brought near the pan, and the weight is measured again. From the difference of weights in and out of the magnetic field, the value of M may be calculated.physicalchemical(can't decide)CA sample of X is carefully weighed and put inside a sealed calorimeter. Pure oxygen gas is injected into the calorimeter, and the mixture ignited. After all of X has reacted with the oxygen gas, the temperature rise of the calorimeter is measured. From this change in temperature the value of C may be calculated.physicalchemical(can't decide)
Explanation:
A chemical property is one in which atoms are rearranged in the process.
-----------------
Q) In this case, this is a chemical property because hydrogen starts being consumed when the flask is heated and hydrogen combines with the solid too.
Chemical
-----------------
M) This is a physical property because nothing happens to the atoms of the different substances in the sample. The metallic particles from the sample are removed with the magnet.
Physical
----------------
C) This is chemical property because a reaction is carried out inside.
Oxygen reacts with X
Chemical
Express your answer is a chemical equations identify all the phases in your answer
We have a reaction between potassium oxide and water. They already present us with the chemical equation but we must balance it.
For this we add the coefficient two in front of the KOH molecule, in this way we will have on each side of the reaction:
K--->2 atoms
O---> 2 atoms
H---> 2 atoms
So, the chemical balanced equation will be:
[tex]K_2O_{(s)}+H_2O_{(l)}\rightarrow2KOH_{(aq)}[/tex]The subscript "s" refers to the solid state, "l" to a liquid state, and "aq" to a solution of the solute in water.