Question

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A...

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g),
Kc = 1.67×10−7 at 800∘C
A 0.500 L reaction vessel initially contains 0.100 mol of H2S and 0.138 mol of  H2 at 800∘C.​

Find the equilibrium concentration of  [S2].

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Dear student,

Please give a positive rating if satisfied with the answer.

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 for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7 at 800∘C The reaction is...
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7 at 800∘C The reaction is carried out at the same temperature with the following initial concentrations: [H2S][H2][S2]===1.20×10−4M0.00M0.00M Find the equilibrium concentration of S2. Express the concentration to three significant figures and include the appropriate units.
the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7 at 800 ∘C The reaction is...
the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7 at 800 ∘C The reaction is carried out at the same temperature with the following initial concentrations: [H2S]=1.90×10−4 M [H2]= 0M [S2]= 0M Find the equilibrium concentration of S2
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g),                            &nbs
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g),                              Kc=1.67×10−7 at 800∘C The reaction is carried out at the same temperature with the following initial concentrations: [H2S] =4.80 x 10^-4 M [H2] = 0.00 M [S2]= 0.00 M Find the equilibrium concentration of S2 . Express the concentration to three significant figures and include the appropriate units.
Consider the following reaction at equilibrium: 2H2(g)+S2(g)⇌2H2S(g)+heat In a 10.0-L container, an equilibrium mixture contains 2.20...
Consider the following reaction at equilibrium: 2H2(g)+S2(g)⇌2H2S(g)+heat In a 10.0-L container, an equilibrium mixture contains 2.20 g of H2, 10.9 g of S2 and 68.1 g of H2S. Part A What is the numerical Kc value for this equilibrium mixture? Part B If more H2 is added to the equlibrium mixture, how will the equilibrium shift? Part C How will the equilibrium shift if the mixture is placed in a 5.00-L container with no change in temperature? Part D If...
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?
At 500 ºC, the decomposition of water into hydrogen and oxygen, 2H2O(g) 2H2(g) + O2(g) has...
At 500 ºC, the decomposition of water into hydrogen and oxygen, 2H2O(g) 2H2(g) + O2(g) has Kc = 6.0 × 10-28. What are the concentrations of H2 and O2 that are present at equilibrium in a 6.00 L reaction vessel at this temperature if the container originally held 0.051 mol H2O? Enter your answer in scientific notation.
When the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.012....
When the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.012. Starting with pure H2S at 1065°, what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g)?
At 800 K, the equilibrium constant, Kp, for the following reaction is 3.2 × 10–7 ....
At 800 K, the equilibrium constant, Kp, for the following reaction is 3.2 × 10–7 . 2 H2S(g) 2 H2(g) + S2(g) A reaction vessel at 800 K initially contains 3.00 atm of H2S. If the reaction is allowed to equilibrate, what is the equilibrium pressure of S2?
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g)+2H2(g)←−→CH3OH(g). An...
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g)+2H2(g)←−→CH3OH(g). An equilibrium mixture in a 1.50 −L vessel is found to contain 7.17×10−2 mol CH3OH, 0.170 mol CO, and 0.301 mol H2 at 500 K. Calculate Kc at this temperature.
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g)+2H2(g)←−→CH3OH(g). An...
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g)+2H2(g)←−→CH3OH(g). An equilibrium mixture in a 1.50 −L vessel is found to contain 7.17×10−2 mol CH3OH, 0.170 mol CO, and 0.301 mol H2 at 500 K. Part A Calculate Kc at this temperature.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT