Be sure to answer all parts. δg o for the reaction h2(g) + i2(g) ⇌ 2hi(g) is 2.60 kj/mol at 25°c. calculate δg, and predict the direction in which the reaction is spontaneous. the initial pressures are: ph2 = 3.10 atm pi2 = 1.5 atm phi = 1.75 atm
δg =
a. the reaction is spontaneous in the forward direction
b. the reaction is spontaneous in the reverse direction
c. cannot be determined
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Ответ:
∆G = 1.567 kJ/mole
The reaction is nonspontaneous., or will be spontaneous in the reverse direction
Explanation:
Step 1: The balanced equation
H2(g) + I2(g) ⇌ 2HI(g) 2.60 kJ/mol at 25°C.
Step 2: Data given
The initial pressures are:
pH2 = 3.10 atm
pI2 = 1.5 atm
pHI = 1.75 atm
Step 3: Calculate Q
Kp = (pHI)^2 / (pH2)(pI2)
Q has the same form but we substitute the non-equilibrium values given in the problem.
Q = (1.75)² / (3.10*1.5) = 0.659
Step 4: Calculate gibbs free energy
∆G = ∆G˚ + RTlnQ = 2600 J/mole + (8.31 J/mole K)(298 K)(ln 0.659) = 2600 J/mole - 1032.729 J/mole
= 1567.271 J/mole = 1.567 kJ/mole
Interpret ∆G:
∆G > 0 the reaction is nonspontaneous., or will be spontaneous in the reverse direction
∆G < 0 the reaction is spontaneous.
If ∆G = 0 the reaction is essentially at equilibrium.
∆G = 1.567 kJ/mole
The reaction is nonspontaneous., or will be spontaneous in the reverse direction
Ответ:
Conduction
Explanation: