Solution Found!
Consider the reaction If 2.0 moles of N2 react with 6.0
Chapter 6, Problem 79P(choose chapter or problem)
Consider the reaction
\(N_{2}(g)+3 H_{2}(g) \rightarrow 2 N H_{3}(g)\)
\(\Delta H_{r x n}^{\circ}=-92.6\ \mathrm{kJ} / \mathrm{mol}\)
If 2.0 moles of \(N_{2}\) react with 6.0 moles of \(H_{2}\) to form \(\mathrm{NH}_{3}\), calculate the work done (in joules) against a pressure of 1.0 atm at \(25^{\circ} \mathrm{C}\). What is \(\Delta U\) for this reaction? Assume the reaction goes to completion.
Questions & Answers
QUESTION:
Consider the reaction
\(N_{2}(g)+3 H_{2}(g) \rightarrow 2 N H_{3}(g)\)
\(\Delta H_{r x n}^{\circ}=-92.6\ \mathrm{kJ} / \mathrm{mol}\)
If 2.0 moles of \(N_{2}\) react with 6.0 moles of \(H_{2}\) to form \(\mathrm{NH}_{3}\), calculate the work done (in joules) against a pressure of 1.0 atm at \(25^{\circ} \mathrm{C}\). What is \(\Delta U\) for this reaction? Assume the reaction goes to completion.
ANSWER:Step 1 of 3
Here, we are going to calculate the work done against pressure 1.0 atm and 25 °C.
Given equation,
= -92.6 kJ/mol
Total moles for reactant = 2 moles +6 moles =8.0 moles
Total moles of product = 4.0 moles
Net loss = 8.0 moles -4.0 moles = 4.0 moles