A quantity of 50 mL of 1.50 M HCl was mixed with 50 mL of 1.50M NaOH in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and NaOH solution was the same, 22.0 oC, and the final temperature of the mixed solution was 32.07oC. Calculate the heat released for the neutralization reaction. NaOH(aq) + HCl(aq) = NaCl(aq) + H2O (l) Assume that the densities and specific heats of the solutions are the same as for water (1.00 g/mL and 4.184 J/g. oC, respectively). a) 2.81 b) -2.81 c) 56.2 d) -4.21 e) -50.2
A quantity of 50 mL of 1.50 M HCl was mixed with 50 mL of 1.50M NaOH in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and NaOH solution was the same, 22.0 oC, and the final temperature of the mixed solution was 32.07oC. Calculate the heat released for the neutralization reaction. NaOH(aq) + HCl(aq) = NaCl(aq) + H2O (l) Assume that the densities and specific heats of the solutions are the same as for water (1.00 g/mL and 4.184 J/g. oC, respectively). a) 2.81 b) -2.81 c) 56.2 d) -4.21 e) -50.2
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section5.6: Calorimetry
Problem 5.7CYU: Assume 200. mL of 0.400 M HCl is mixed with 200. mL of 0.400 M NaOH in a coffee-cup calorimeter The...
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A quantity of 50 mL of 1.50 M HCl was mixed with 50 mL of 1.50M NaOH in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and NaOH solution was the same, 22.0 oC, and the final temperature of the mixed solution was 32.07oC. Calculate the heat released for the neutralization reaction.
NaOH(aq) + HCl(aq) = NaCl(aq) + H2O (l)
Assume that the densities and specific heats of the solutions are the same as for water (1.00 g/mL and 4.184 J/g. oC, respectively).
a) 2.81
b) -2.81
c) 56.2
d) -4.21
e) -50.2
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