The equilibrium constant, Kp, for the following reaction is 55.6at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.33 atm, are introduced into an evacuated vessel at 698 K. PH2 = atm PI2 = atm PHI = atm
The equilibrium constant, Kp, for the following reaction is 55.6at 698 K:
H2(g) + I2(g) 2HI(g)
Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.33 atm, are introduced into an evacuated vessel at 698 K.
| PH2 | = | atm |
| PI2 | = | atm |
| PHI | = | atm |
The equilibrium constant, Kp, for the following reaction is 1.80×10-2 at 698 K:
2HI(g) H2(g) + I2(g)
Calculate the equilibrium partial pressures of all species when HI(g) is introduced into an evacuated flask at a pressure of 1.64 atm at 698 K.
| PHI | = atm |
| PH2 | = atm |
| PI2 | = atm |
A student ran the following reaction in the laboratory at 297 K:
2NOBr(g) 2NO(g) + Br2(g)
When he introduced NOBr(g) at a pressure of 0.292 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of Br2(g) to be 8.43×10-2 atm.
Calculate the equilibrium constant, Kp, he obtained for this reaction.
Kp =
A student ran the following reaction in the laboratory at 304 K:
2NO(g) + Br2(g) 2NOBr(g)
When she introduced NO(g) and Br2(g) into a 1.00 L evacuated container, so that the initial partial pressure of NO was 1.15 atm and the initial partial pressure of Br2 was 0.531 atm, she found that the equilibrium partial pressure of Br2 was 0.228 atm.
Calculate the equilibrium constant, Kp, she obtained for this reaction.
Kp =
Carbon tetrachloride can be produced by the following reaction:
CS2(g) + 3 Cl2(g) ⇄ S2Cl2(g) + CCl4(g)
In an experiment, 0.120 mol of CS2 and 0.360 mol of Cl2 were placed in a 1.00-L flask at a particular temperature. After equilibrium has been achieved, the mixture contains 0.030 mol CCl4. Calculate the value of K under the experimental conditions.
K =
The equilibrium constant, Kp , for the following reaction is 0.110at 298 K.
NH4HS(s) NH3(g) + H2S(g)
If an equilibrium mixture of the three compounds in a 4.64 L container at 298 K contains 2.15 mol of NH4HS(s) and 0.120mol of NH3(g), the partial pressure of H2S(g) is atm.
The equilibrium constant, Kp , for the following reaction is 0.215at 673 K.
NH4I(s) NH3(g) + HI(g)
If an equilibrium mixture of the three compounds in a 5.71 L container at 673 K contains 1.55 mol of NH4I(s) and 0.266mol of NH3(g), the partial pressure of HI(g) is atm.
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