A certain chemical reaction releases 479 kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.36 J of heat energy to raise the temperature of this calorimeter by 1Â°C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 9.9Â°C.

a. How would you calculate the number of moles of reactant that were consumed?

Question

Damien

Chemistry

13 January, 06:12

A certain chemical reaction releases 479 kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.36 J of heat energy to raise the temperature of this calorimeter by 1Â°C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 9.9Â°C.

a. How would you calculate the number of moles of reactant that were consumed?

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Answers (1)

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Zara Perkins · Answer 1

6.94 x 10^-5 mol

Explanation:

It takes 3.36 J of heat energy to raise the temperature of this calorimeter by 1Â°C.

The temperature of the calorimeter is found to rise by 9.9Â°C.

So how much energy was required to achieve this?

3.36 J = 1Â°C

x = 9.9Â°C

x = 9.9 * 3.36 / 1

x = 33.264 J

The chemical reaction releases 479 kJ of heat energy per mole of reactant consumed.

So number of moles consumed is given as;

479000 J = 1

33.264 J = x

x = 33.264 J * 1 / 479000J

x = 6.94 x 10^-5 mol