Question

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 reaction 3A ⇌ 2B + C The equilibrium concentration of gas C is 0.125 mol/L. Determine the equilibrium concentration of gas A.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
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.
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
1.575 mol N2O3 is put into a 2.00 L flask at 25°C where it decomposes into...
1.575 mol N2O3 is put into a 2.00 L flask at 25°C where it decomposes into NO2(g) and NO(g). What is the equilibrium constant (to 4 decimal places) if the reaction mixture contains 0.300 mol NO2 at equilibrium?
H2 + I2 <---> 2HI Kp=100 Initially, a flask contains hydrogen gas at 0.010atm iodine gas...
H2 + I2 <---> 2HI Kp=100 Initially, a flask contains hydrogen gas at 0.010atm iodine gas at 0.0050atm, and hydorgen iodide gas at 0.50atm. Determine equilibrium partial pressure of each gas in the flask.
For the reaction given below, 2.00 moles of A and 3.00 moles of B are placed...
For the reaction given below, 2.00 moles of A and 3.00 moles of B are placed in a 6.00-L container. A(g) + 2B(g) C(g) At equilibrium, the concentration of A is 0.220 mol/L. What is the value of K? (6.90)
A 4.0L reaction flask initially contains 4.0 mol of SO3 at 400K. Sulfur dioxide and oxygen...
A 4.0L reaction flask initially contains 4.0 mol of SO3 at 400K. Sulfur dioxide and oxygen form: 2SO3(g) ↔ 2SO2(g) + O2(g). After equilibrium is established, 0.27 mol SO3 remain. What is the value of Kc?
Introduced into a 1.50 L flask is 0.100 mol PCl5(g). The flask is held at 227°C...
Introduced into a 1.50 L flask is 0.100 mol PCl5(g). The flask is held at 227°C until equilibrium is established. What are the partial pressures and the total pressure of the gases in the flask at equilibrium? PCl5(g) ↔ PCl3(g) + Cl2(g) 1) Calculate ∆H°rxn 2) Calculate ∆S°rxn 3) Calculate Keq 4) Calculate Pinitial (PCl5) 5) Calculate equilibrium pressures for PCl5(g), PCl3(g), Cl2(g) 6) calculate total pressure of this gas mixture at equilibrium
1. Suppose we fill a sealed flask with 0.250 mol of gas A, which then completely...
1. Suppose we fill a sealed flask with 0.250 mol of gas A, which then completely reacts to form a second gas, B, according to the reaction: A → 2B. At various times during the reaction, we measure the amount of B in the flask and get the following data: Time (s) 0.00 30.0 60.0 90.0 120 Moles of B 0.000 0.167 0.278 0.350 0.400 a. Calculate the number of moles of A remaining in the flask at each time...
Dinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4(g) → 2NO2(g) A 1.000-L flask is...
Dinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4(g) → 2NO2(g) A 1.000-L flask is charged with 3.00 × 10-2 mol of N2O4. At equilibrium, 2.36 × 10-2 mol of N2O4 remains. Keq for this reaction is ________. I am wondering why you do not have to convert the moles to molality to solve this problem?
A mixture initially contains A, B, and C in the following concentrations: [A]=0.700mol L−1, [B]=1.05mol L−1,...
A mixture initially contains A, B, and C in the following concentrations: [A]=0.700mol L−1, [B]=1.05mol L−1, and [C]=0.550mol L−1. The following reaction occurs and equilibrium is established: A(aq)+2B(aq)⇌C(aq) At equilibrium, [A]=0.550mol L−1 and [C]=0.700mol L−1. Calculate the value of the equilibrium constant, Kc .
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT