A certain chemical reaction 444 kj releases 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 of heat energy to raise the temperature of this calorimeter by . Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by . How would you calculate the number of moles of reactant that were consumed

Complete question is;

A certain chemical reaction 444 kj releases 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 4.68 J of heat energy to raise the temperature of this calorimeter by 6.9 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by . How would you calculate the number of moles of reactant that were consumed

7.27 × 10^(-5) moles

Explanation:

We are given;

Heat energy = 444 kJ/mol

Final Temperature = 6.9 °C

Heat capacity = 4.68 J/°C

Let's calculate the heat generated from the formula;

Heat generated = heat capacity × final temperature

Heat generated = 4.68 × 6.9 = 32.292 J = 32.292 × 10^(-3) KJ

Now, the number of moles of reactant that were consumed is gotten from;

No_ of moles of rctnt consumed = heat energy generated/heat energy used = (32.292 × 10^(-3))/444 = 7.27 × 10^(-5) moles