When 25 ml of 1 M H 2 SO 4 is added to 50ml of 1 M NaOH at 25 C in a calorimeter

Question

When 25 ml of 1 M H2SO4 is added to 50ml of 1 M NaOH at 25 C in a calorimeter, the temp of the aqueous solution increases to 33.9 C. Assuming the specific heat os the solution is 4.18 (J/gC), that its density is 1 g/ml, and that the calorimeter itself absorbs a negligibkle ammount of heat, calculate delta H in kJ for the rxn:

H2SO4 (aq) + 2NaOH(s) -> 2H2O (l) + Na2SO4 (aq)

this question was answered in here and the answer is going to be 112kj/mol. however, what I dont understand is why we only considered the moles of H2SO4 to calculate the enthalpy of the reaction. why did not we use the 2NaOH to find the enthalpy?

Explanation / Answer

In this they only considered H2SO4 for calculation but NaOH since on calculation delta H , only aquas and gaseous state are considered , solid state is not considered

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