A student mixes two water solutions with an initial temperature of 25 degrees Celsius to form a final solution with a mass of 65.0 g at 30.0 degrees Celsius. What is the heat change in kJ for this reaction

Heat change = 3.77kJ

Explanation:

T1 = 25°C

Mass = 65g

T2 = 30°C

specific heat capacity of water = 4.184J/g°C

Heat energy = ?

Heat energy = MC∇T

Heat energy (Q) = MC(T2 - T1)

Q = 65 * 4.184 * (30 - 15)

Q = 251.04 * 15

Q = 3765.6J

Q = 3.77KJ

The heat change during the reaction was 3.77kJ

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.