Problem: 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

🤓 Based on our data, we think this question is relevant for Professor Gray's class at CSU.

FREE Expert 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.


View Complete Written Solution
Problem Details

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