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Chapter 5: Q30E (page 227)

When 1.0g of fructose, C6H12O6(s), a sugar commonly found in fruits, is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by 1.58˚C. If the heat capacity of the contents is 9.90kJ/˚C, what is q for this combustion?

Short Answer

Expert verified

The heat of combustion for this reaction is 15.6 kJ.

Step by step solution

01

Given data

Data we are provided with:

The mass of the fructose = 1.0 g

The increase in the temperature (∆T) = +1.58˚C

The heat capacity of the calorimeter(C) = 9.90 kJ/˚C

02

Heat of combustion

The formula that is used in finding the heat of the combustion (q) in a bomb calorimeter is

C × ∆T.

The heat of the combustion = 9.90 KJ/˚C × 1.58˚C

= 1.56 kJ

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Most popular questions from this chapter

Calculate \[{\bf{\Delta H}}_{{\bf{298 }}}^{\bf{^\circ }}\] for the process \[{\bf{C}}{{\bf{o}}_{\bf{3}}}{{\bf{O}}_{\bf{4}}}\left( {\bf{s}} \right) \to {\bf{3Co}}\left( {\bf{s}} \right){\bf{ + 2}}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right)\]

from the following information:

\[\begin{array}{c}{\bf{Co(s) + }}\frac{{\bf{1}}}{{\bf{2}}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}} \to {\bf{CoO(s) \Delta H}}_{{\bf{298}}}^{\bf{^\circ }}{\bf{ = - 237}}{\bf{.9kJ}}\\{\bf{3CoO(s) + }}\frac{{\bf{1}}}{{\bf{2}}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}} \to {\bf{C}}{{\bf{o}}_{\bf{3}}}{{\bf{O}}_{\bf{4}}}{\bf{(s) \Delta H}}_{{\bf{298}}}^{\bf{^\circ }}{\bf{ = - 177}}{\bf{.5kJ}}\end{array}\]

Which of the enthalpies of combustion in Table 5.2 the table are also standard enthalpies of formation?

Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter (Figure 5.12) at 22.4°C causes the temperature to rise to 25.8°C. What is the approximate amount of heat involved in the dissolution, assuming the heat capacity of the resulting solution is 4.18 J/g°C? Is the reaction exothermic or endothermic?

How many milliliters of water at 23 °C with a density of 1.00 g/mL must be mixed with 180 mL (about 6 oz) of coffee at 95 °C so that the resulting combination will have a temperature of 60 °C? Assume that coffee and water have the same density and the same specific heat.

Ethanol, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\), is used as a fuel for motor vehicles, particularly in Brazil.

(a) Write the balanced equation for the combustion of ethanol to CO2(g) and H2O(g), and, using the data in Appendix G, calculate the enthalpy of combustion of 1 mole of ethanol.

(b) The density of ethanol is 0.7893 g/ml. Calculate the enthalpy of combustion of exactly 1 L of ethanol.

(c) Assuming that an automobile’s mileage is directly proportional to the heat of combustion of the fuel, calculate how much farther an automobile could be expected to travel on 1 L of gasoline than on 1 L of ethanol. Assume that gasoline has the heat of combustion and the density of n–octane, \({{\bf{C}}_{\bf{8}}}{{\bf{H}}_{{\bf{18}}}}\) (ΔHf=

- 208.4 kJ/mol; density = 0.7025 g/mL).
See all solutions

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