A certain chemical reaction releases 497.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 4.32J of heat energy to raise the temperature of this calorimeter by 1°C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 12.8°C. 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.
Question
A certain chemical reaction releases 497.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 4.32J of heat energy to raise the temperature of this calorimeter by 1°C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 12.8°C. 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.
Solution
The number of moles of reactant consumed can be calculated using the formula:
n = (q_calorimeter / q_reaction)
where:
- q_calorimeter is the heat absorbed by the calorimeter, which can be calculated as (C_calorimeter * ΔT), where C_calorimeter is the heat capacity of the calorimeter (4.32 J/°C) and ΔT is the change in temperature (12.8°C).
- q_reaction is the heat released per mole of reactant, which is given as 497 kJ/mol.
So, the expression becomes:
n = ((C_calorimeter * ΔT) / q_reaction)
Substituting the given values:
n = ((4.32 J/°C * 12.8°C) / 497 kJ/mol)
Note: Be careful with the units. The heat capacity is given in J/°C and the heat of reaction is given in kJ/mol. You may need to convert units for these quantities to match.
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