This question is incomplete, the complete question is;
What is the heat of a reaction, in joules, with a total reaction mixture volume of 73.0 mL if the reaction causes a temperature change of 4.4 °C in a calorimeter?
Assume that the reaction mixture has a density of 1.00 g/mL and a specific heat of 4.184 J/g-oC. The calorimeter has a heat capacity of 10.0 J/oC.
Answer: the heat of the reaction is 1387.9 J
Explanation:
Given that;
Volume = 73.0 mL
density = 1.00 g/mL
specific heat of solution = 4.184 J/g-oC
calorimeter has a heat capacity of 10.0 J/oC.
Temperature change ΔT = 4.4 °C
the heat of a reaction = ?
Total heat of the reaction will be equal to the amount of heat absorbed/lost by the solution and the calorimeter.
so heat of reaction q = mC_solΔT + C_alΔT
where m is mass, C_sol is specific heat capacity of the solution, ΔT temperature change and C_cal is heat capacity of calorimeter.
so first we calculate our mass;
mass = volume × density
= 73.0 mL × 1.00 g/mL
= 73.0 g
so we substitute into our equation;
q = mC_solΔT + C_alΔT
q = (73 × 4.184 × 4.4) + ( 10 × 4.4 )
q = 1343.9008 + 44
q = 1387.9 J
Therefore the heat of a reaction is 1387.9 J
