At a certain temperature, Kp = 4.5 x 103 for the reaction: 2H2S(g) ⇌ 2H2(g)...

Question

Question

At a certain temperature, K_p = 4.5 x 10³ for the reaction:

2H₂S(g) ⇌ 2H₂(g) + S₂(g)

If P[H₂S] = 0.0050 atm, P[H₂] = 0.50 atm, and P[S₂] = 0.75 atm, then

answer choices:

Q_p < K_p and the reaction will shift toward products.

Q_p < K_p and the reaction will shift toward reactants

Q_p > K_p and the reaction will shift toward products.

Q_p = K_p and the reaction is at equilibrium.

Q_p > K_p and the reaction will shift toward reactants.

science chemistry

Answer 1

Answer #1

Ginen! P[H25] = 0.005 atm p[H2] = 0.5 atm P[s₂] - 015 atm 2 H23(g) + 2H2(g) +52(9) Qp, P [12 ] p[s,] (0.5)*x (0.75) P[H₂S]² 3

Answer 2

Similar Homework Help Questions

At a certain temperature, Kp = 4.5 x 103 for the reaction: 2H2S(g) = 2H2(g) +...

At a certain temperature, Kp = 4.5 x 103 for the reaction: 2H2S(g) = 2H2(g) + S2(g) If P[H2S] = 0.0050 atm, P[H2] = 0.50 atm, and P[S2] = 0.75 atm, then Qp > Kp and the reaction will shift toward products. O Qp > Kp and the reaction will shift toward reactants. O Qp <Kp and the reaction will shift toward products. O Qp = Kp and the reaction is at equilibrium. Qp <Kp and the reaction will shift...
1. Which of the following conditions defines a non-spontaneous oxidation-reduction reaction? E° + ΔG° - &

1. Which of the following conditions defines a non-spontaneous oxidation-reduction reaction? E° + ΔG° - Keq <1 E° - ΔG° - Keq <1 E° + ΔG°+ Keq >1 E° + ΔG°- Keq >1 E° - ΔG° + Keq <1 2. What information can be obtained from the Figure below? The equivalence point occurs at pH = 7.0 but the pKa is not known from the graph. Both the pOH and the...
8. If the reaction 2H2S(g) = 2H2(g) + S2(g) is carried out at 1065°C, Kp =...

8. If the reaction 2H2S(g) = 2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.0120. Starting from pure H2S introduced into an evacuated vessel at 1065°C, what will the total pressure in the vessel at equilibrium if the equilibrated mixture contains 0.300 atm of H2(g)? Answer 1.51 atm (1.5 pts)

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) = 2H2(g) + S2(g), Kc =...

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) = 2H2(g) + S2(g), Kc = 1.67 x 10-7 at 800°C The reaction is carried out at the same temperature with the following initial concentrations: [H2S] [H2] [S2] 4.00 x 10-4M 0.00 M 0.00 M - Part A Find the equilibrium concentration of S2. Express the concentration to three significant figures and include the appropriate units. HA ? [S2] = Value Units
The following reaction 2H2S(g)⇌2H2(g)+S2(g),Kc=1.654×10−7 at 800∘C is carried out at the same temperature with the following...

The following reaction 2H2S(g)⇌2H2(g)+S2(g),Kc=1.654×10−7 at 800∘C is carried out at the same temperature with the following initial concentrations: [H2S]=0.132M, [H2]=0.165 M, and [S2]=0.00 M. Find the equilibrium concentration of S2. Express the molarity to three significant figures. Answer in units of nM.
The following reaction 2H2S(g)⇌2H2(g)+S2(g),Kc=1.619×10−7 at 800∘C is carried out at the same temperature with the following...

The following reaction 2H2S(g)⇌2H2(g)+S2(g),Kc=1.619×10−7 at 800∘C is carried out at the same temperature with the following initial concentrations: [H2S]=0.069M, [H2]=0.059 M, and [S2]=0.00 M. Find the equilibrium concentration of S2. Express the molarity to three significant figures. Answer in units of nM.

At a particular temperature, Kc = 1.6 x 10-2 for 2H2S(g) -- 2H2(g) + S2(g). Initially,...

At a particular temperature, Kc = 1.6 x 10-2 for 2H2S(g) -- 2H2(g) + S2(g). Initially, only H2S is present in a reaction vessel. When solving for equilibrium concentrations, which initial concentration of H25 will X-is-small approximation work? 1.10 M 0.105 M 12.0 M
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g) Kc = 1.67×10^-7 at 800∘C The...

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]=1.00×10^−4M [H2]=0.00M [S2]=0.00M Part A 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...

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]=3.20×10-4M [H2]=0.00M [S2]=0.00M Find the equilibrium concentration of S2. Express the concentration to three significant figures and include the appropriate units.

At 1130°C, the equilibrium constant (Kc) for the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is 2.25...

At 1130°C, the equilibrium constant (Kc) for the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is 2.25 × 10−4. If [H2S] = 4.60 × 10−3 M and [H2] = 1.70 × 10−3 M, calculate [S2]. × 10 M (Enter your answer in scientific notation.)