when 50.08 g of 1.00 m naoh at 23 c is added to 50.22 g of 1.00 m hcl at 23 c, the resulting temperature of the mixture is 29.7 c. (assume that the calorimeter constant is equal to zero. assume that the solutions have the same specific heat capacity (4.184 j/g·k) and density (1.00 g/ml) as water. take care with signs.)

a) what is δt for this process?

b) calculate qsolution (in j) for this process.

c) calculate qreaction (in j) for this process

d) calculate the moles of naoh and the moles of hcl used in the reaction. determine whether naoh or hcl is the limiting reactant.

e) what is the enthalpy change (δhrxn, in kj/mol) for this process per mol of the limiting reactant?

f) is the reaction of naoh with hcl an endothermic or exothermic process?