Solution Found!
Given the thermochemical equations: calculate the for the
Chapter 6, Problem 74P(choose chapter or problem)
Given the thermochemical equations:
\(B r_{2}(l)+F_{2}(g) \rightarrow 2 B r F(g)\)
\(\Delta H^{\circ}=-188\ \mathrm{kJ} / \mathrm{mol}\)
\(B r_{2}(l)+3 F_{2}(g) \rightarrow 2 B r F_{3}(g)\)
\(\Delta H^{\circ}=-768\ \mathrm{kJ} / \mathrm{mol}\)
calculate the \(\Delta H_{r x n}^{\circ}\) for the reaction
\(B r F(g)+F_{2}(g) \rightarrow B r F_{3}(g)\)
Questions & Answers
QUESTION:
Given the thermochemical equations:
\(B r_{2}(l)+F_{2}(g) \rightarrow 2 B r F(g)\)
\(\Delta H^{\circ}=-188\ \mathrm{kJ} / \mathrm{mol}\)
\(B r_{2}(l)+3 F_{2}(g) \rightarrow 2 B r F_{3}(g)\)
\(\Delta H^{\circ}=-768\ \mathrm{kJ} / \mathrm{mol}\)
calculate the \(\Delta H_{r x n}^{\circ}\) for the reaction
\(B r F(g)+F_{2}(g) \rightarrow B r F_{3}(g)\)
ANSWER:Step 1 of 4
Here, we are going to calculate the for the reaction.
Given that
= -188 kJ/mol ---(1)
=-768 kJ/mol ---(2)