/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Q5.3-75E The white pigment \({\bf{Ti}}{{\... [FREE SOLUTION] | 91影视

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Chapter 5: Q5.3-75E (page 273)

The white pigment \({\bf{Ti}}{{\bf{O}}_{\bf{2}}}\)is prepared by the reaction of titanium tetrachloride, \({\bf{TiC}}{{\bf{l}}_{\bf{4}}}\), with water vapor in the gas phase:

\({\bf{TiC}}{{\bf{l}}_{\bf{4}}}\left( {\bf{g}} \right){\bf{ + 2}}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right) \to {\bf{Ti}}{{\bf{O}}_{\bf{2}}}\left( {\bf{s}} \right){\bf{ + 4HCl}}\left( {\bf{g}} \right)\)

How much heat is evolved in the production of exactly 1 mole of \({\bf{Ti}}{{\bf{O}}_{\bf{2}}}\)(s) under standard state conditions?

Short Answer

Expert verified

The amount of heat evolved during the production of exactly one mole of TiO2(s) will be 66.388 kJ.

Step by step solution

01

Enthalpy of formation of substances

To calculate the amount of heat evolved in the production of exactly one mole of TiO2(s), we have to know the formation enthalpy of each compound involved in the reaction. The reaction is:

\({\rm{TiC}}{{\rm{l}}_{\rm{4}}}\left( {\rm{g}} \right){\rm{ + 2}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{g}} \right) \to {\rm{Ti}}{{\rm{O}}_{\rm{2}}}\left( {\rm{s}} \right){\rm{ + 4HCl}}\left( {\rm{g}} \right)\)

\(\begin{array}{l}{\rm{The enthalpy of formation of TiC}}{{\rm{l}}_{\rm{4}}}\left( {\rm{g}} \right){\rm{ is }} - 763.2{\rm{ kJ/mol}}{\rm{.}}\\{\rm{The enthalpy of formation of }}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{g}} \right){\rm{ is }} - 241.82{\rm{ kJ/mol}}{\rm{.}}\\{\rm{The enthalpy of formation of Ti}}{{\rm{O}}_2}\left( {\rm{g}} \right){\rm{ is }} - 944{\rm{ kJ/mol}}{\rm{.}}\\{\rm{The enthalpy of formation of HCl}}\left( {\rm{g}} \right){\rm{ is }} - 92.307{\rm{ kJ/mol}}{\rm{.}}\end{array}\)

02

Enthalpy of reaction

\(\begin{array}{l}{\rm{Enthalpy of reaction, }}\\{\bf{\Delta }}{{\bf{{\rm H}}}_{{\bf{reaction}}}}{\bf{ = }}\sum {{\bf{\Delta }}{{\bf{{\rm H}}}_{{\bf{products}}}}} {\bf{ - }}\sum {{\bf{\Delta }}{{\bf{{\rm H}}}_{{\bf{reactants}}}}} \\{\rm{\Delta }}{{\rm{{\rm H}}}_{{\rm{reaction}}}}{\rm{ = }}\left( {{\rm{4 \times \Delta }}{{\rm{{\rm H}}}_{{\rm{HCl}}\left( {\rm{g}} \right)}}{\rm{ + \Delta }}{{\rm{{\rm H}}}_{{\rm{Ti}}{{\rm{O}}_{\rm{2}}}\left( {\rm{g}} \right)}}} \right){\rm{ - }}\left( {{\rm{\Delta }}{{\rm{{\rm H}}}_{{\rm{TiC}}{{\rm{l}}_{\rm{4}}}\left( {\rm{g}} \right)}}{\rm{ + 2 \times \Delta }}{{\rm{{\rm H}}}_{{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{g}} \right)}}} \right)\\{\rm{\Delta }}{{\rm{{\rm H}}}_{{\rm{reaction}}}}{\rm{ = }}\left( {{\rm{4 \times - 92}}{\rm{.307 + - 944}}} \right){\rm{ - ( - 763}}{\rm{.2 - 2 \times 241}}{\rm{.82)}}\\{\rm{\Delta }}{{\rm{{\rm H}}}_{{\rm{reaction}}}}{\rm{ = }}\left( {{\rm{ - 1313}}{\rm{.228}}} \right){\rm{ + }}\left( {{\rm{1246}}{\rm{.84}}} \right){\rm{ kJ}}\\{\rm{\Delta }}{{\rm{{\rm H}}}_{{\rm{reaction}}}}{\rm{ = - 66}}{\rm{.388 kJ}}\end{array}\)

Hence, the amount of heat evolved during the production of exactly one mole of TiO2(s) will be 66.388 kJ.

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Most popular questions from this chapter

Ethylene, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}\), a byproduct from the fractional distillation of petroleum, is fourth among the 50 chemical compounds produced commercially in the largest quantities. About 80% of synthetic ethanol is manufactured from ethylene by its reaction with water in the presence of a suitable catalyst. \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}{\bf{(g) + }}{{\bf{H}}_{\bf{2}}}{\bf{O(g)}} \to {{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH(l)}}\).Using the data in the table inAppendix G, calculate 螖H掳 for the reaction.

Question: How much heat, in joules and in calories, must be added to a 75.0鈥揼 iron block with a specific heat of 0.449 J/g 掳C to increase its temperature from 25 掳C to its melting temperature of 1535 掳C?

A 92.9-g piece of a silver/gray metal is heated to 178.0 掳C, and then quickly transferred into 75.0 mL of water initially at 24.0 掳C. After 5 minutes, both the metal and the water have reached the same temperature: 29.7 掳C. Determine the specific heat and the identity of the metal. (Note: You should find that the specific heat is close to that of two different metals. Explain how you can confidently determine the identity of the metal).

A 70.0-g piece of metal at 80.0 掳C is placed in 100 g of water at 22.0 掳C contained in a calorimeter like that shown in Figure 5.12. The metal and water come to the same temperature at 24.6 掳C. How much heat did the metal give up to the water? What is the specific heat of the metal?

Question 11: A piece of unknown solid substance weighs 437.2 g, and requires 8460 J to increase its temperature from 19.3 掳C to 68.9 掳C.

(a) What is the specific heat of the substance?

(b) If it is one of the substances found in Table 5.1, what is its likely identity?
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