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Chapter 5: Question 15 E (page 269)

Would the amount of heat measured for the reaction in example 5.5be greater, lesser, or remain the same if we used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your answer.

Short Answer

Expert verified

The amount of heat measured would be lesser if the calorimeter was replaced with a poorly insulated calorimeter.

Step by step solution

01

Change in temperature

The amount of heat measured inexample 5.5 is 2.89kJ.

If the calorimeter is poorly insulated, it will lose heat to its surroundings, decreasing the overall temperature of the reaction.Therefore, the change in temperature would also decrease.

02

Heat measured

The heat required to raise the temperature of a substance is given by the formula Q = C\( \times \)m\( \times \)\(\Delta \)T, where“C” is thespecific heat of the substance, “m” is the mass of the substance, and “∆T” is the change in the temperature of the substance.

Suppose the change in temperature decreases, and the heat measured for the reaction would also decrease. So, the heat measured for the reaction in example 5.5 would be less than 2.89kJ.

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Most popular questions from this chapter

If a reaction produces 1.506 kJ of heat, which is trapped in 30.0 g of water initially at 26.5 °C in a calorimeter like that in Figure 5.12, what is the resulting temperature of the water?

The addition of 3.15g of Ba(OH)2.8H2O to a solution of 1.52g of NH4SCN in 100g of water in a calorimeter caused the temperature to fall by 3.1˚C. Assuming the specific heat of the solution and products is 4.20J/g˚C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation:
Ba(OH)2.8H2O(s) + 2NH4SCN (aq) -------> Ba(SCN)2(aq) + 2NH3(aq) + 10H2O(l)

A piece of unknown metal weighs 217 g. When the metal piece absorbs 1.43 kJ of heat, its temperature increases from 24.5 °C to 39.1 °C. Determine the specific heat of this metal and predict its identity.

In the early days of automobiles, illumination at night was provided by burning acetylene, C2H2. Though no longer used as auto headlamps, acetylene is still used as a source of light by some cave explorers. The acetylene is (was) prepared in the lamp by the reaction of water with calcium carbide, CaC2:

\({\bf{Ca}}{{\bf{C}}_{\bf{2}}}\left( {\bf{s}} \right){\bf{ + 2}}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{l}} \right) \to {\bf{Ca}}{\left( {{\bf{OH}}} \right)_{\bf{2}}}\left( {\bf{s}} \right){\bf{ + }}{{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{2}}}\left( {\bf{g}} \right)\)

Calculate the standard enthalpy of the reaction. The \({\bf{\Delta H}}_{\bf{f}}^{\bf{o}}\)of CaC2is -15.14 kcal/mol.

How much heat is produced by combustion of 125 g of methanol under state conditions?
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