Solution Found!
Consider the reaction If 2.0 moles of H2O(g) are converted
Chapter 6, Problem 27P(choose chapter or problem)
Consider the reaction
\(\begin{aligned}2 \mathrm{H}_{2} \mathrm{O}(g) \longrightarrow & 2\mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \\\Delta H &=483.6 \mathrm{~kJ} / \mathrm{mol}\end{aligned}\)
If \(2.0\) moles of \(\mathrm{H}_{2} \mathrm{O}(g)\) are converted to \(\mathrm{H}_{2}(g)\) and \(\mathrm{O}_{2}(g)\) against a pressure of \(1.0\) atm at \(125^{\circ} \mathrm{C}\), what is \(\Delta U\) for this reaction?
Questions & Answers
QUESTION:
Consider the reaction
\(\begin{aligned}2 \mathrm{H}_{2} \mathrm{O}(g) \longrightarrow & 2\mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \\\Delta H &=483.6 \mathrm{~kJ} / \mathrm{mol}\end{aligned}\)
If \(2.0\) moles of \(\mathrm{H}_{2} \mathrm{O}(g)\) are converted to \(\mathrm{H}_{2}(g)\) and \(\mathrm{O}_{2}(g)\) against a pressure of \(1.0\) atm at \(125^{\circ} \mathrm{C}\), what is \(\Delta U\) for this reaction?
ANSWER:Step 1 of 2
The goal of the problem is to calculate \(\Delta U\) for this reaction given.
Given reaction:
\(2 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g)\)
Given:
\(\Delta H=483.6 \mathrm{~kJ} / \mathrm{mol}\)
Number of moles of \(\mathrm{H}_{2} \mathrm{O}=2.0 \text { moles }\)
Pressure (P) = 1.0 atm
Temperature (T) = \(125^{\circ} \mathrm{C}\)
\(\Delta U\) is calculated using the formula shown below:
\(\Delta U=\Delta H-R T \Delta n\)
where \(\Delta H\) = change in enthalpy.
R = gas constant = 8.314 J/mol?K
T = Temperature
n = number of moles