Answer:
-241.826 kJ·mol⁻¹; -146.9 J·K⁻¹mol⁻¹; 664.6 J·K⁻¹mol⁻¹; spontaneous
Explanation:
½O₂(g) + H₂(g) ⟶ H₂O(g)
ΔHf°/kJ·mol⁻¹: 0 0 -241.826
S°/J·K⁻¹mol⁻¹: 205.0 130.6 188.7
1. ΔᵣH
ΔᵣH = products -reactants = -241.826 -(0 + 0) = -241.826 kJ·mol⁻¹
2. ΔᵣS
ΔᵣS = products - reactants = 188.7 - (205.0 + 130.6) = 188.7 - 335.6 = -146.9 J·K⁻¹mol⁻¹
3. ΔS(univ)

4. Spontaneity

ΔG is negative, so the reaction is spontaneous.
The value for ΔG = 18 kJ/mol
<h3>Further explanation</h3>
Given
ΔH = 27 kJ/mol and ΔS = 0.09 kJ/mol.K
T = 100 K
Required
the value for ΔG
Solution
The spontaneous process of a reaction is based on 2 factors :
- enthalpy change ΔH decreases and
- entropy change ΔS increases
ΔG=ΔH-T.ΔS

Answer:
Remove a H2 molecule from the left side of the equation.
Explanation:
i took the quiz and got it right
If 1mole ------------- is ---------------- 6.02*10²³
than 0.25mole ----- is ---------------- x
x = [0.25mole*6.02*10²³]/1mole = <u>1,505*10²³</u>
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