## Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning

# Chapter 4 - Energy and Chemical Reactions - Questions for Review and Thought - Topical Questions - Page 189e: 76b

#### Answer

$Ti(s) + 2Cl_2(g) -- \gt TiCl_4(l)$ $\Delta_fH^{\circ}\{TiCl_4(l)\} = -804.2kJ/mol$

#### Work Step by Step

1. Write the separated atoms, and their coefficients, to form a single $NH_3$ $Ti + 4Cl -- \gt TiCl_4$ 2. Analyze the appendix J, and find the standard state for each element: - Hint: It is the compound with $\Delta_fH^{\circ}$ = 0. - Divide the coefficient by the number of atoms in each compound in standard state: $\frac{1}{1} Ti(s) + \frac{4}{2}Cl_2(g) -- \gt TiCl_4(l)$ Just add the $\Delta_fH^{\circ}$** after the reaction. ** Appendix J. $Ti(s) + 2Cl_2(g) -- \gt TiCl_4(l)$ $\Delta_fH^{\circ}\{TiCl_4(l)\} = -804.2kJ/mol$

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