To determine change in Gibbs Free Energy, we use the equation
ΔG = ΔG° + RT ln Q
where ΔG is the change in free energy at temperature T
ΔG° is the free energy at standard temperature
R is the universal gas constant
T is the temperature of the system
Q is the reaction quotient
First, we determine the reaction quotient. It is the ratio of the concentration or partial pressure of the products and the reactants. For this case, we do as follow:
<span>P2(g) + 3 Cl2(g) -> 2 PCl3(g)
</span>
<span>Q = P(PCl3) ^2 / (P(P2)(P(Cl2 ^ 3)))
</span>Q = (0.65 atm)^2 / (1.5 atm) (1.6 atm)^3
Q = 0.0688
Substituting to the equation for free energy,
ΔG = ΔG° + RT ln Q
ΔG = -33300 J/mol + (8.314 J/mol-K)(298 K) ln 0.0688
ΔG = -39931.35 J/mol
According to your question seems like Block E is densest. Hope it helps
Answer:
The answer to your question is: letter B
Explanation:
First, write the reactions and balance them
a. 2 CH3OH + 3 O2 ⇒ 2 CO2 + 4 H2O
ratio 3/2 = 1.5
b. 2 CH2 = CHCH3 + 9 O2 ⇒ 3 CO2 + 3 H2O
ratio 9/2 = 4.5
c. 2 CH ≡ CH + 5 O2 ⇒ 4 CO2 + 2 H2O
ratio 5/2 = 2.5
Answer:
ok so first of all try working hard then ill answer u
Explanation: