Question

For the reaction 2A(g) ⇌ B(g) + C(g) at 700 °C, Kc = 1.61. Calculate the...

For the reaction
2A(g) ⇌ B(g) + C(g)
at 700 °C, Kc = 1.61. Calculate the number of moles of B present at equilibrium if 3.32 moles of A is heated to 700 °C in a 9.56-L container.

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
For the reaction 2A(g) + B(s) ⇌ C(g) + D(g) at 700 °C, Kc = 0.0389....
For the reaction 2A(g) + B(s) ⇌ C(g) + D(g) at 700 °C, Kc = 0.0389. Calculate the number of moles of C present at equilibrium if a mixture of 3.55 moles of C and 3.55 moles of D is heated to 700 °C in a 5.85-L container.
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180×106 at 730°...
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180×106 at 730° C. Starting with 4.20 moles of HBr in a 17.8−L reaction vessel, calculate the concentrations of H2,Br2, and HBr at equilibrium. 17. The equilibrium constant Kc for the reaction below is 0.00771 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0433 M and [Br] = 0.0462 M, calculate the concentrations of these species at equilibrium. For the reaction...
A.) For the reaction 2A(g)+2B(g)⇌C(g) Kc = 56.8 at a temperature of 341 ∘C . Calculate...
A.) For the reaction 2A(g)+2B(g)⇌C(g) Kc = 56.8 at a temperature of 341 ∘C . Calculate the value of Kp. B.For the reaction X(g)+3Y(g)⇌2Z(g) Kp = 2.60×10−2 at a temperature of 301 ∘C . Calculate the value of Kc.
Compound A decomposes to B and C according to the following equations: 2A(g) doubleheadarrow B(g) +...
Compound A decomposes to B and C according to the following equations: 2A(g) doubleheadarrow B(g) + 3C(g) At 100 degree C, 1.41 mol of A were placed in a 5.50 L container, and the reaction was allowed to proceed. After equilibrium was established, it was found that 65.9% of A has decomposed. What is the value of Kc for this reaction at 100 degee C?
For the reaction 2A(g) + B(s) ? C(g) + D(g) at 700
For the reaction 2A(g) + B(s) ? C(g) + D(g) at 700
Hydrogen sulfide decomposes according to the following reaction, for which Kc = 9.30 10-8 at 700°C....
Hydrogen sulfide decomposes according to the following reaction, for which Kc = 9.30 10-8 at 700°C. 2 H2S(g) 2 H2(g) + S2(g) If 0.33 mol H2S is placed in a 2.6 L container, what is the equilibrium concentration of H2(g) at 700°C?
Part A For the reaction 2A(g)+2B(g)⇌C(g) Kc = 62.6 at a temperature of 187 ∘C ....
Part A For the reaction 2A(g)+2B(g)⇌C(g) Kc = 62.6 at a temperature of 187 ∘C . Calculate the value of Kp. Express your answer numerically. --------------------------------- Part B For the reaction X(g)+3Y(g)⇌3Z(g) Kp = 3.10×10−2 at a temperature of 325 ∘C . Calculate the value of Kc. Express your answer numerically.
For the reaction: 2H2O(g) ⇌ 2H2(g) + O2(g) KC = 2.40 x 10-3 at a given...
For the reaction: 2H2O(g) ⇌ 2H2(g) + O2(g) KC = 2.40 x 10-3 at a given temperature. At equilibrium, it is found that [H2O] = 0.294 M and [H2] = 1.80 x 10-2 M. If the reaction is run in a 5.50 L container, how many moles of O2 are present at equilibrium?
The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g)...
The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 6.80 L container at 548 K contains 2.48 mol of NH4Cl(s) and 0.307 mol of NH3, the number of moles of HCl present is moles.
The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s)-----> NH3(g)...
The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s)-----> NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 6.21 L container at 298 K contains 3.17 mol of NH4HS(s) and 0.335 mol of NH3, the number of moles of H2S present is ____ moles??
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT