Question

Additional Problem 6.098 Your answer is partially correct. Try again. A dilute solution of hydrochloric acid with a mass of 614.08 g and containing 0.30664 mol of HCl was exactly neutralized in a calorimeter by the sodium hydroxide in 618.91 g of a comparably dilute solution. The temperature increased from 16.663 to 19.946 °C. The specific heat of the HCl solution was 4.031 Jug-1.°C-1; that of the NaOH solution was 4.046 Jug-1.00-1. The heat capacity of the calorimeter was 77.99 j.oc-1. Enter the balanced equation for the reaction. Include states in your answer. HCl(aq) + NaOH(aq) —H2O(l) + NaCl(aq) Edit Use the data above to calculate the heat evolved. What is the heat of neutralization per mole of HCI? Assume that the original solutions made independent contributions to the total heat capacity of the system following their mixing. AH = kJ/mol the tolerance is +/-2%

Answer 1

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for HCL (9) = mSAT = 614:08 gm x 4.031.54cx (19.946-161663) °c 3 8126-60J for NOSH (2) = mSAT = 618.91 gm x 4.046 Fox (19.946- 16.663)°C = 8221.0J for calorieneter 122) = Sx4T = 77.99 3% x (19.946 -166639°c = 256.04 J. Total heat eralved (@ =9,+92 +92 = 8126.60 +8221.0 + 256.04 = 16603.643 AH = heat lostlevalved - - 16603-645 = 54147-01J moles of Her 0.3066amol mor AH = -54.15 kJ/ -ve sign as heat is evolved. Mo