Question

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)?

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
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), 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.
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...
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].
Consider the reaction: N2(g) + 3H2(g) → 2NH3(g). At a particular moment during the reaction hydrogen...
Consider the reaction: N2(g) + 3H2(g) → 2NH3(g). At a particular moment during the reaction hydrogen is being consumed at a rate of 0.074 M/s. At this moment: (a) What is the rate of reaction (in M/s)? {3 points} (b) A what rate (in M/s) is NH3 being produced? {3 points} (c) Are these average or instantaneous rates? {1 point} [3] A certain first-order reaction has a rate constant of 1.65 min-1 at 20°C. What is the value of the...
1) The following reaction was carried out in a 2.25 L reaction vessel at 1100 K:...
1) The following reaction was carried out in a 2.25 L reaction vessel at 1100 K: C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 8.75 mol of C, 14.1 mol of H2O, 3.60 mol of CO, and 8.50 mol of H2, what is the reaction quotient Q? 2) The following reaction was performed in a sealed vessel at 782 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.65M and...
1. Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.25 −L flask at a...
1. Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.25 −L flask at a certain temperature contains 26.8 g CO and 2.35 g H2. At equilibrium, the flask contains 8.64 g CH3OH. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. 2. Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1358 torr and a H2O partial pressure of 1764 torr at 2000 K....
1. The equilibrium constant for the chemical equation is Kp = 21.8 at 179 °C. Calculate...
1. The equilibrium constant for the chemical equation is Kp = 21.8 at 179 °C. Calculate the value of the Kc for the reaction at 179 °C. 2. At a certain temperature, the Kp for the decomposition of H2S is 0.822. H2S(g)--->H2(g)+S(g) Initially, only H2S is present at a pressure of 0.120 atm in a closed container. What is the total pressure in the container at equilibrium?
A) The reaction of CH4 is carried out at a different temperature with an initial concentration...
A) The reaction of CH4 is carried out at a different temperature with an initial concentration of [CH4]= 9.1�10?2M . At equilibrium, the concentration ofH2 is 2.0�10?2M . 2CH4(g)?C2H2+3H2(g). Find the equilibrium constant at this temperature. B) The reaction between CO and H2 is carried out at a different temperature with initial concentrations of[CO] = 0.35M and [H2]= 0.60M . CO(g)+2H2(g)?CH3OH(g) At equilibrium, the concentration of CH3OH is 0.12M . Find the equilibrium constant at this temperature.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT