the following reaction occurred in a calorimeter: h2SO4 (aq) +2 naoh(aq) ----->

Question

the following reaction occurred in a calorimeter:
h2SO4 (aq) +2 naoh(aq) -----> na2so4 (aq) +2 h2o
(a) 50 ml of 2.00 M naoh and 50.0 ml of 1.00M h2so4 were placed in a calorimeter. the the temperature of the solution increased from 22.5c to 36.1 c.
assume that the density of the initial solutions is 1.00 g/ml and the specific heat of the final solution is 4.18 j/gc
calculate the change of heat of the reaction in kj/mol h2so4.
(b) use your answer to (a) and the data in appendix c to calculate change of heat H (f) of na2so4 (aq)

Explanation / Answer

Q1.

mol of NaOH = MV = 50*2 = 100 mmol of NaOH

mmol of H2SO4 = MV = 50*1 = 50 mmol of H2SO4

ratio si 1:2 so this is fine, equal ratio

dT = 36.1-22.5 = 13.6

total mass = 50 + 50 = 100 mL --> 100 g

C = 4.184 J/gC

Qmix = m*C*(Tf-Ti) = 100*4.184*13.6 = 5690.24 J

now, calculated HRxn

HRxn = -Q/mol = -(5690.24)/(100*10^-3) = -56902.4 J/mol = -56.9 kJ/mol

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