equation for q

[Sristi Palimar 2E]

In class, we learned that q = n*c*deltaT or q = g*c*delta t. However, the achieve solutions manual often shows calculations for q using the equation q = c*deltaT. For example, for problem 4D.3:

4D.3 The reaction of 1.40 g of carbon monoxide with excess water vapor to produce carbon dioxide and hydrogen gases in a bomb calorimeter causes the temperature of the calorimeter assembly to rise from 22.113 celsius to 22.799 celsius. The calorimeter assembly is known to have a total heat capacity (calorimeter constant) of
3 KJ/celsius. Calculate the internal energy change, deltaU , for the reaction of 1 mol CO(g).

To determine the q of the calorimeter, the solution manual uses q = c*deltaT. Why is the mass of the calorimeter not given/needed to solve for q?

[Chem_Mod]

This textbook problem gives you the TOTAL HEAT CAPACITY of the calorimeter rather than the SPECIFIC HEAT CAPACITY. Remember we discussed in lecture that heat capacity is energy needed to raise the temperature of a substance by 1 K. Specific heat capacity is the energy needed to raise temperature of ONE GRAM of a substance by 1 K. Therefore if total heat capacity rather than specific heat capacity is given, one does not need to factor in mass (g) as it is already factored in the heat capacity itself