Rate = k[A] = first order reaction
<h3>Further explanation</h3>
Given
Rate law
Required
A first-order reaction
Solution
The rate law : equation for the rate of chemical reaction
For reaction
aA + bB ⇒ C
The rate : r = k[A]ᵃ[B]ᵇ
The sum of exponents(a+b) is the reaction order
From the choice :
a. a+b = 2, second order reaction
b. a+b = 3, third order reaction
c. a+b = 4, fourth order reaction
d a+0 = 1, first order reaction
Answer:
ΔG = 2721.891 J/mol
Explanation:
- C2H4(g) + H2O(g) ↔ C2H5OH(g)
∴ ΔH°rxn = - 45.8 KJ/mol
∴ Kp = 28.5
If p(C2H4) = p(H2O) = p(C2H5OH) = 3.0 atm ⇒ ΔG°rxn = ?
⇒ Kp = (PC2H5OH/P*) / (PC2H4/P*)(PH2O/P*)
∴ P* = 1 atm
⇒ Kp = (3 atm) / (3 atm)(3 atm) = 0.33
⇒ Ln Kp = - ΔG/RT
⇒ ΔG = - RT LnKp
∴ T = 298 K
∴ R = 8.314 J/mol.K
⇒ ΔG = - ((8.314 J/mol.K)(298 K)) Ln(0.33)
⇒ ΔG = 2721.891 J/mol
