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a} Define the term standard enthalpy change of neutralisation. b) The enthalpy change of reaction between NaHCO3 and HCI was determined experimentally. 3.50 g of NaHCO3 (M, = 84.0) and 50 cm³ of 1.0 mol dm 3 HCI (aq) were mixed at time = 2 min, and several temperature readings were taken at fixed intervals. Fig. 1 shows the graph of temperature against time. Using the information from the graph and assuming that the specific heat capacity and density of all solutions are 4.18 J g1K-1 and 1.00 g cm-3 respectively, calculate the enthalpy change of the reaction: NaHCO3 (s) + HCI (aq) NaCI (aq) + H2O (1) + CO2 (g) State one assumption used in your calculation.

a} Define the term standard enthalpy change of neutralisation. b) The enthalpy change of reaction between NaHCO3 and HCI was determined experimentally. 3.50 g of NaHCO3 (M, = 84.0) and 50 cm³ of 1.0 mol dm 3 HCI (aq) were mixed at time = 2 min, and several temperature readings were taken at fixed intervals. Fig. 1 shows the graph of temperature against time. Using the information from the graph and assuming that the specific heat capacity and density of all solutions are 4.18 J g1K-1 and 1.00 g cm-3 respectively, calculate the enthalpy change of the reaction: NaHCO3 (s) + HCI (aq) NaCI (aq) + H2O (1) + CO2 (g) State one assumption used in your calculation.

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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a) Define the term standard enthalpy change of neutralisation. b) The enthalpy change of reaction between NaHCO3 and HCI was determined experimentally. 3.50 g of NaHCO3 (M, = 84.0) and 50 cm3 of 1.0 mol dm-3 HCI (aq) were mixed at time = 2 min, and several temperature readings were taken at fixed intervals. Fig. 1 shows the graph of temperature against time. Using the information from the graph and assuming that the specific heat capacity and density of all solutions are 4.18 J g-1 K-1 and 1.00 g cm-3 respectively, calculate the enthalpy change of the reaction: NaHCO3 (s) + HCI (aq) → NaCI (aq) + H2O (I) + CO2 (g) - State one assumption used in your calculation.
Transcribed Image Text:a) Define the term standard enthalpy change of neutralisation. b) The enthalpy change of reaction between NaHCO3 and HCI was determined experimentally. 3.50 g of NaHCO3 (M, = 84.0) and 50 cm3 of 1.0 mol dm-3 HCI (aq) were mixed at time = 2 min, and several temperature readings were taken at fixed intervals. Fig. 1 shows the graph of temperature against time. Using the information from the graph and assuming that the specific heat capacity and density of all solutions are 4.18 J g-1 K-1 and 1.00 g cm-3 respectively, calculate the enthalpy change of the reaction: NaHCO3 (s) + HCI (aq) → NaCI (aq) + H2O (I) + CO2 (g) - State one assumption used in your calculation.
20 18 16 temperature / °C 14 12- 10 10 12 time / minutes Fig. 1 c) The enthalpy change of neutralisation of HCl with NaOH is given to be -57.3 kJ mol-1. The following information is given: NaHCO3(s) + aq→ NaHCO3(aq); AH = +17.6 kJ mol-1 By using these information and your answer to (b), construct an energy cycle and calculate AH. for the reaction: CO2(g) + NaOH(aq) → NaHCO3(aq) d) A similar experiment carried out with hydrogen cyanide, HCN(aq), and aqueous ammonia gave a value of -5.4 kJ mol-1 for the enthalpy change of neutralisation. The corresponding value for sodium hydroxide with hydrochioric acid was -57.0 kJ mol-1. Suggest a possible explanation for the difference in these two values.
Transcribed Image Text:20 18 16 temperature / °C 14 12- 10 10 12 time / minutes Fig. 1 c) The enthalpy change of neutralisation of HCl with NaOH is given to be -57.3 kJ mol-1. The following information is given: NaHCO3(s) + aq→ NaHCO3(aq); AH = +17.6 kJ mol-1 By using these information and your answer to (b), construct an energy cycle and calculate AH. for the reaction: CO2(g) + NaOH(aq) → NaHCO3(aq) d) A similar experiment carried out with hydrogen cyanide, HCN(aq), and aqueous ammonia gave a value of -5.4 kJ mol-1 for the enthalpy change of neutralisation. The corresponding value for sodium hydroxide with hydrochioric acid was -57.0 kJ mol-1. Suggest a possible explanation for the difference in these two values.
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