Question

1. In an experiment, 3.00 mol of iodine gas and 3.00 mol of chlorine gas are...

1. In an experiment, 3.00 mol of iodine gas and 3.00 mol of chlorine gas are initially placed into a 4.00 L container at 225°C. Construct an ICE table and find the concentrations of all reactants and products at equilibrium. [A5]


I2 (g) + Cl2 (g) ⇌ 2 ICl (g) K = 44.6 at 225°C

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Please like the answer if you find it helpful. I did the best I could .

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298...
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2=0.35 atm and PCl2=0.35 atm . What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298...
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2=0.40 atm and PCl2=0.40 atm . What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?
Calculate the equilibrium concentrations of 12.00 mol iodine gas and 8.00 mol hydrogen gas for the...
Calculate the equilibrium concentrations of 12.00 mol iodine gas and 8.00 mol hydrogen gas for the production of hydrogen iodide gas in a 4.00 Liter vessel. The K = 86.5 Please use ICE method
1. Consider 1.20 mol of carbon monoxide and 4.00 mol of chlorine sealed in a 6.00...
1. Consider 1.20 mol of carbon monoxide and 4.00 mol of chlorine sealed in a 6.00 L container at 476 oC. The equilibrium constant, Kc, is 2.50 (in M-1) for CO(g) + Cl2(g) ? COCl2(g) Calculate the equilibrium molar concentration of CO. 2. For the reaction in the previous problem, that is, 2HI(g) ? H2(g) + I2(g) Keq = 0.016 Initially a container contains 0.40 M HI and no product. What is the equilibrium concentration of H2?
At a certain temperature the equilibrium constant, K c, equals 0.11 for the reaction: 2 ICl(g)...
At a certain temperature the equilibrium constant, K c, equals 0.11 for the reaction: 2 ICl(g) ↔ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.25 mol of I2 and 0.25 mol of Cl2 are initially mixed in a 2.0-L flask?
CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 464...
CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 464 ∘C . At equilibrium, the concentrations were measured and the following results obtained: Gas Partial Pressure (atm) CO 0.780 Cl2 1.22 COCl2 0.120 What is the equilibrium constant, Kp, of this reaction? Part B The following reaction was performed in a sealed vessel at 767 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.75M and [I2]=2.05M. The equilibrium concentration...
Hydrogen reacts with chlorine to form an equilibrium with hydrogen chloride gas. A mixture of 3.50...
Hydrogen reacts with chlorine to form an equilibrium with hydrogen chloride gas. A mixture of 3.50 mole each of hydrogen and chlorine is placed in an 8.00 L container and allowed to reach equilibrium. If the equilibrium constant Kc is 1.23 at this temperature, what are the concentrations of hydrogen, chlorine, and hydrogen chloride (in that order and in molarity) at equilibrium? H2 (g) + Cl2 (g) ⇌ 2 HCl (g) K = 1.23 Question 8 options: 0.271, 0.271, 0.167...
A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B....
A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B. Gas A       decomposes according to the following reaction:     3A 2B + C The equilibrium concentration of gas C is 0.131 mol/L. Determine the value of the equilibrium constant, K.
Part A Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane,...
Part A Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane, CH3C5H9, according to the equation: C6H12 ↔ CH3C5H9 If K c = 0.143 at 25°C for this reaction, find the equilibrium concentrations of C6H12 and CH3C5H9 if the initial concentrations are 0.200 M and 0.150 M, respectively. Part B Consider the following reaction: CuS(s) + O2(g) ↔ Cu(s) + SO2(g) A reaction mixture initially contains 2.9 M O2. Determine the equilibrium concentration of O2...
Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes...
Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 468 ∘C . At equilibrium, the concentrations were measured and the following results obtained: Gas Partial Pressure (atm) CO 0.760 Cl2 1.25 COCl2 0.170 What is the equilibrium constant, Kp, of this reaction...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT