🤓 Based on our data, we think this question is relevant for Professor Gray's class at CSU.
Solution: Given the following reactionsH2O (l) →H2O (g) ΔH = 44.01 kJ2H2 (g) + O2 (g) → 2H2O (g) ΔH = -483.64 kJthe enthalpy for the decomposition of liquid water into gaseous hydrogeand oxygen2H2O (l) → 2H2 (g) + O2 (g) is __________ kJ.A) -395.62B) -527.65C) 439.63D) 571.66E) 527.65
Problem
Given the following reactions
H2O (l) →H2O (g) ΔH = 44.01 kJ
2H2 (g) + O2 (g) → 2H2O (g) ΔH = -483.64 kJ
the enthalpy for the decomposition of liquid water into gaseous hydrogeand oxygen
2H2O (l) → 2H2 (g) + O2 (g)
is __________ kJ.
A) -395.62
B) -527.65
C) 439.63
D) 571.66
E) 527.65
Solution
We’re being asked to determine the enthalpy change (ΔHrxn) for the chemical reaction:
2 H2O (l) → 2 H2 (g) + O2 (g)
We can use Hess’s Law to determine the enthalpy change of the overall reaction from the given reactions:
1. H2O (l) →H2O (g) ΔH1 = 44.01 kJ
2. 2H2 (g) + O2 (g) → 2H2O (g) ΔH2 = - 483.64 kJ
We now need to find a combination of reactions that when added up, gives us the overall reaction.
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