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

a. qrxn = 831 J

b. 863 J

Explanation:

we know that density is the mass of a substance per unit volume

d=mass/volume

the volume of the solution is the combination of solution A and solution B

1.02 g/mL=mass/(25+25)

mass=50*1.02

mass=51g

Recall that Q=mCdT

mass=m, C=specific heat capacity

dT=change in temperature

qrxn = (51 g)(4.18 J/g⋅°C)(25.3 °C - 21.4 °C)

qrxn = 831 J

2.Heat=Heat capacity *change in temperature

qcal = (8.20 J/°C)((25.3 °C - 21.4 °C)

qcal = 31.98 J

qrxni + qcal = qrxn

qrxn = 831 J + 32.0 J

863 J Heat of reaction

863 J =(51 g)(Heat Capacity)(25.3 °C - 21.4 °C)

4.34 J/g⋅°C

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: