Question

If 8.0 g of NH4HS(s) is placed in a sealed vessel with a volume of 1.0...

If 8.0 g of NH4HS(s) is placed in a sealed vessel with a volume of 1.0 L and heated to 200 ∘C the reaction NH4HS(s) ⇌ NH3(g) + H2S(g) will occur. When the system comes to equilibrium, some NH4HS(s) is still present. Which of the following changes will lead to a reduction in the amount of NH4HS(s) that is present, assuming in all cases that equilibrium is re-established following the change? If 8.0 of is placed in a sealed vessel with a volume of 1.0 and heated to 200 the reaction will occur. When the system comes to equilibrium, some is still present. Which of the following changes will lead to a reduction in the amount of that is present, assuming in all cases that equilibrium is re-established following the change?

Increasing the volume of the vessel

Adding more H2S(g) to the vessel

Decreasing the volume of the vessel

Adding more NH4HS(s) to the vessel

Adding more NH3(g) to the vessel

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
Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction NH4HS(s)⇌NH3(g)+H2S(g) This reaction...
Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction NH4HS(s)⇌NH3(g)+H2S(g) This reaction has a Kp value of 0.120 at 25 ∘C.In addition to the H2S already present in the flask, solid NH4HS is added until there is excess unreacted solid remaining. A) What are the partial pressures of NH3 and H2S at equilibrium, that is, what are the values of PNH3 and PH2S, respectively? B) What is the mole fraction, χ, of H2S in the gas...
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??
Consider the reaction: NH4HS (s) --> NH3 (g) + H2S (g). At a certain temperature, Kc...
Consider the reaction: NH4HS (s) --> NH3 (g) + H2S (g). At a certain temperature, Kc = 8.5 * 10^-3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?
he equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g)...
he 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 7.52 L container at 298 K contains 3.52 mol of NH4HS(s) and 0.300 mol of NH3, the number of moles of H2S present is ? Please help do not eve know where to start with this
The equilibrium constant (Kp) for the reaction below is 70.0 at 32 °C: NH4HS(s) <---> NH3(g)...
The equilibrium constant (Kp) for the reaction below is 70.0 at 32 °C: NH4HS(s) <---> NH3(g) + H2S(g) A sample of NH4HS(s) is placed in an evacuated container and allowed to come to equilibrium. (You should calculate what the P is of all gases at this point) The partial pressure of H2S is then increased by the addition of 1.00 bar of H2S, and the system responds accordingly( shifts?). Calculate the partial pressure of every gas after such shift.
consider the following equilibrium at 395K: NH4HS (s) <--> NH3 (g) + H2S (g) the partial...
consider the following equilibrium at 395K: NH4HS (s) <--> NH3 (g) + H2S (g) the partial pressure of each gas is 0.397 atm, what is the value of Kp and Kc?
The equilibrium constant, K, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) +...
The equilibrium constant, K, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.231 mol NH4HS, 1.34×10-2 M NH3 and 1.34×10-2 M H2S. If the concentration of H2S(g) is suddenly increased to 2.08×10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M [H2S] = M please finish it...
When 0.100 mol of CaCO3(s) and 0.100 mol of CaO(s) are placed in an evacuated, sealed...
When 0.100 mol of CaCO3(s) and 0.100 mol of CaO(s) are placed in an evacuated, sealed 10.0−L container and heated to 385 K, PCO2 = 0.220 atm after equilibrium is established: CaCO3(s) ⇌ CaO(s) + CO2(g) An additional 0.290 atm of CO2(g) is pumped in. What is the total mass (in g) of CaCO3 after equilibrium is reestablished?
5.80 mol of solid A was placed in a sealed 1.00-L container and allowed to decompose...
5.80 mol of solid A was placed in a sealed 1.00-L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.20 M, where it remained constant. A(s)=B(g)+C(g) Then, the container volume was doubled and equilibrium was re-established. How many moles of A remain?​
5.60 mol of solid A was placed in a sealed 1.00-L container and allowed to decompose...
5.60 mol of solid A was placed in a sealed 1.00-L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s) <---> B(g) + C(g) Then, the container volume was doubled and equilibrium was re-established. How many moles of A remain?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT