If the density of nitrogen gas at a certain pressure and temperature is 1.20 g/l, how many moles of nitrogen gas are in 15.0 l
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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.