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

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