A50.0 ml sample of a 1.00 m solution of cuso4 is mixed with 50.0 ml of 2.00 m koh in a calorimeter. the temperature of both solutions was 20.2 degree celsious before mixing and 26.3 degree celsious after mixing . the heat capacity of the calorimeter is 12.1 j/k. from the data, calculate delta hfor the process
cuso4(1 m)+2koh(2 (oh)2(s)+k2so4(0.5 m)
assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the volumes are additive.

Answer : The enthalpy change for the process is 52.5 kJ/mole.

Explanation :

Heat released by the reaction = Heat absorbed by the calorimeter + Heat absorbed by the solution

where,

q = heat released by the reaction

= heat absorbed by the calorimeter

= heat absorbed by the solution

= specific heat of calorimeter =

= specific heat of water =

= mass of water or solution =

= change in temperature =

Now put all the given values in the above formula, we get:

Now we have to calculate the enthalpy change for the process.

where,

= enthalpy change = ?

q = heat released = 2626.61 J

n = number of moles of copper sulfate used =

Therefore, the enthalpy change for the process is 52.5 kJ/mole.

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa