A certain chemical reaction releases 362.kj of heat energy per mole of reactant consumed. Suppose some moles of the reactant are

Question

2 months ago

10

A certain chemical reaction releases 362.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 4.87j of heat energy to raise the temperature of this calorimeter by 5.5 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?
Set the math up. But don't do any of it. Just leave your answer as a math expression.

Also, be sure your answer includes all the correct unit symbols.

Chemistry

1 answer:

lions [2.9K] · Answer 1 · 2026-02-18T22:18:55+03:00

Answer:

The temperature increase of the calorimeter, which is missing in the problem, is necessary for the calculation.

Explanation:

Since the temperature rise (X) is unspecified, we'll express the calculation in terms of X, and demonstrate with an example value.

1) Calorimeter details:

Temperature increase: X °C

Heat capacity ratio: 4.87 J / 5.5 °C (given)

Energy absorbed by calorimeter at X °C rise:

(4.87 J / 5.5 °C) × X

2) Reaction data:

Heat released: 362 kJ per mole of reactant

Number of moles consumed: n

Total energy from reaction:

362 kJ/mol × 1000 J/kJ × n = 362,000 n J

3) Using energy conservation, assuming no heat loss to surroundings, the energy from the reaction equals the energy absorbed by the calorimeter:

362,000 n = (4.87 J / 5.5 °C) × X

Solving for n gives:

n = [(4.87 / 5.5) × X] / 362,000

n = 0.000002446 × X

This means for each degree Celsius rise in calorimeter temperature, 0.000002446 moles of reactant were consumed.

Example:

If the calorimeter temperature increases by 100 °C, then:

n = 0.000002446 × 100 = 0.0002446 mol