Calculating Heat Produced in a Chemical Reaction

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To calculate the heat produced in the reaction, first determine the number of moles of Cl2 produced, which is given as 0.0100 mol. The reaction's enthalpy change (ΔrH) is -202 kJ per mole of Cl2 formed. Multiply the moles of Cl2 by the enthalpy change to find the total heat produced, resulting in q(system) = 0.0100 mol * -202 kJ/mol = -2.02 kJ, or -2020 J. The temperature change is not necessary for this calculation since the heat produced is directly derived from the reaction's enthalpy. Thus, the heat produced in the system is -2020 J.
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Homework Statement


OCl–(aq) + Cl–(aq) + 2H+(aq) Cl2(aq) + H2O ΔrH = -202 kJ mol–1
25.0mL of a solution 0.400mol L–1 in both OCl– and Cl– was reacted with excess hydrochloric acid. The mass of the solution after mixing was 100 g.
n(reaction) = 0.0100 mol

Find q(system) in joules.
Assume that the temperature change of the vessel in which the experiment is carried out is negligible
Assume that the heat capacity of the mixture is the same as the specific heat capacity of water (4.184 J g–1 K–1).

Homework Equations

I know somewhere you have to use the formula q = mcΔT but I am unsure what to do because there is no temperature in the question.

The Attempt at a Solution



I have tried multiplying the mass and temp change but I think i am wrong. Please help?
 
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It is not about q = mcΔT.

You are told how much heat is produced per mole of produced Cl2. How many moles were produced?
 

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