Answer:
1.71x10²⁷
Explanation:
If we sum 1/2 of (3) + 1/2 of (1):
1/2 (3.) C(s) + 1/2O₂(g) ⇌ CO(g), K₃ = √2.10×10⁴⁷ = 4.58x10²³
1/2 (1) 1/2CO₂(g) + 3/2H₂(g) ⇌ 1/2CH₃OH(g) + 1/2H₂O(g), K₁ = √1.40×10² = 11.8
C(s) + 1/2O₂(g) +<u> 1/2CO₂(g) </u>+<u> 3/2H₂(g</u>) ⇌ 1/2CH₃OH(g) + <u>1/2H₂O(g)</u> + <u>CO(g)</u>
K' = 4.58x10²³ * 11.8 = 5.42x10²⁴
+1/2 (2):
<u>1/2 CO(g)</u> +<u> 1/2H₂O(g)</u> ⇌<u> 1/2CO₂(g)</u> + <u>1/2H₂</u> (g), K = √1.00×10⁵ = 316.2
C(s) + 1/2O₂(g) + H₂(g) ⇌ 1/2 CHO₃H(g) + 1/2CO(g)
K'' = 5.42x10²⁴* 316.2 =
<h3>1.71x10²⁷</h3>
For the reaction c2h6 (g) → c2h4 (g) + h2 (g) δh° is 137 kj/mol and δs° is 120 j/k ∙ mol. the reaction is spontaneous at high temperatures. the correct answer is option(b).
A spontaneous reaction is one that favors the creation of products in the environment in which it is taking place. A campfire that is roaring is an exothermic example of a spontaneous reaction (there is a decrease in the energy of the system as energy is released to the surroundings as heat).
There are some reactions that are only spontaneous at very high temperatures according to the Gibbs Free Energy equation. The reaction is spontaneous at high temperatures if both S, or entropy, and H, or enthalpy, are positive. We want the Gibbs free energy to be negative according to the formula G = H - T - S.
The complete question is:
For the reaction
C2H6 (g) → C2H4 (g) + H2 (g)
ΔH° is +137 kJ/mol and ΔS° is +120 J/K ∙ mol. This reaction is ________.
A) spontaneous at all temperatures
B) spontaneous only at high temperature
C) spontaneous only at low temperature
D) nonspontaneous at all temperatures
To know more about spontaneous reaction refer to: brainly.com/question/1217654
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Answer:
C. Hold polar molecules together.
Explanation:
This is just something you have to know.