The specific heat of a solution is 4.18 j/(g•°c)and its density is 1.02 g/ml. the solution is formed by combining 25.0 ml of solution a with 25.0 ml of solution b with each solution initially at 21.4°c. the final temperature of the combined solution is 25.3°c. calculate the heat of reaction, q, assuming no heat loss due to the calorimeter.
i got 831 j
the part i cannot figure out is the question afterwards which is if the calorimeter has a heat capacity of 8.20 j/°c and a correction is included to account for the heat absorbed by the calorimeter what is the heat of reaction q

Okay, so, to solve for this, we're going to have to use q = mcΔT. However, the mass of the calorimeter is not important because not of it is used in the reaction, so really, we are only looking at 2 things, the temperature change and specific heat. So, here is the lightly modified equation we will use:
q = cΔT

Now, just plug in the ΔT we had for the original equation (which was 3.9) and use the specific heat of the calorimeter to get q.

q = (8.20) * (3.9)
q = 31.98, or about 32

The 32 is what was absorbed by the calorimeter, so we can add that to the original value to get our answer.
831 + 32 = 863 J

So, the answer is 863 J

Hope this helped!! :D

Iwould you figure it out but you don't have a picture or in your question as to what the physical property you're looking for is