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 oC in a calorimeter

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.

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

c. heat could easily travel through the molecules in the air and escape/enter the flask. removing the air slows down the heat transfer.  

i'm assuming that the correct answer is indeed the first one/ "a"..