A quantity of 2.00 × 102 mL of 0.715 M HCl is mixed with 2.00 ×...
A quantity of 2.00 × 102 mL of 0.715 M HCl
is mixed with 2.00 × 102 mL of 0.358 M
Ba(OH)2 in a constant-pressure calorimeter of negligible
heat capacity. The initial temperature of the HCl and
Ba(OH)2 solutions is the same at 20.29°C. For the
process
H+(aq) + OH−(aq) → H2O(l)
the heat of neutralization is −56.2 kJ/mol. What is the final
temperature of the mixed solution?
Homework Answers
A quantity of 2.00 x 102 mL of 0.745 M HCl is mixed with 2.00 102...
A quantity of 2.00 x 102 mL of 0.745 M HCl is mixed with 2.00 102 mL of 0.373 M Ba(OH), in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.02°C. For the process ht(aq) + OH(aq) + H2O(1) the heat of neutralization is -56.2 kJ/mol. What is the final temperature of the mixed solution? 1 °C
Enter your answer in the provided box. A quantity of 2.00 x 102 mL of 0.807...
Enter your answer in the provided box. A quantity of 2.00 x 102 mL of 0.807 M HCl is mixed with 2.00 10mL of 0.404 M Ba(OH), in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.19°C. For the process H*(aq) + OH(aq) + H2O(1) the heat of neutralization is --56.2 kJ/mol. What is the final temperature of the mixed solution?
Enter your answer in the provided box. A quantity of 2.00 x 102 mL of 0.477...
Enter your answer in the provided box. A quantity of 2.00 x 102 mL of 0.477 M HCl is mixed with 2.00 x 102mL of 0.239 M Ba(OH), in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.45°C. For the process below, the heat of neutralization is -56.2 kJ/mol. What is the final temperature of the mixed solutions? H(aq) + OH(aq) H20(1).
10. A quantity of 2.00 x 102 mL of 0.862 M HCl (mw: 36.46 g/mol) is...
10. A quantity of 2.00 x 102 mL of 0.862 M HCl (mw: 36.46 g/mol) is mixed with 2.00 x 102 mL of 0.431 M Ba(OH)2 (mw: 171.34 g/mol) in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.48 °C. Given, H+(aq) + OH-(aq) + H2O(1) AH° = -56.2 kſ/mol what is the final temperature (°C) of the mixed solution? Assume the solution mixture has a density of...
A quantity of 8.00 102 mL of 0.600 M HNO3 is mixed with 8.00 102 mL...
A quantity of 8.00 102 mL of 0.600 M HNO3 is mixed with 8.00 102 mL of 0.300 M Ba(OH2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNOs reacts with 0.500 mol Ba(OH)2 is-56.2 kJ/mol Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and·184 J/g·? respectively). What is the final...
a quantity of 300 mL of 0.8 M HCl is mixed with 300mL of 0.4 M...
a quantity of 300 mL of 0.8 M HCl is mixed with 300mL of 0.4 M Ba(OH)2 in a constant pressure calorimeter having a heat capacity of 415 J/degrees C. the initial temperature of both solutions is the same at 22.0 degrees C. Given that the specific heat of the solution is 4.184J/g degrees C the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H^+(aq)+OH^-(aq)->H2O (1) is -56.2 kJ/mol, what is the...
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of...
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC, the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH" (aq) - H20 (1) is -56.2...
help 2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL...
help
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC. the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH(aq) → H20 (1) is -56.2...
Please help 2. Two solutions namely, 500 mL of 0.50 M HCl and 500 mL of...
Please help
2. Two solutions namely, 500 mL of 0.50 M HCl and 500 mL of 0.50 M NaOH at the same temperature of 21.6 °C are mixed in a constant-pressure calorimeter. The heat capacity of the calorimeter was 450 J/oC. Given that the specific heat of the solution is 4.184 J/g°C, the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H* (aq) + OH (aq) -- H2O (1) is -56.2 kJ,...
A quantity of 12.0 mL of 6.00 M HBr is mixed with 12.0 mL of 6.00...
A quantity of 12.0 mL of 6.00 M HBr is mixed with 12.0 mL of 6.00 M NaOH in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 21.30°C. The heat of neutralization when 1.00 mol of HBr reacts with 1.00 mol NaOH is -56.1 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water (1,00 g/mL and 4.184 °C. respectively). What is the final...
A quantity of 2.00 x 102 mL of 0.745 M HCl is mixed with 2.00 102 mL of 0.373 M Ba(OH), in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.02°C. For the process ht(aq) + OH(aq) + H2O(1) the heat of neutralization is -56.2 kJ/mol. What is the final temperature of the mixed solution? 1 °C
Enter your answer in the provided box. A quantity of 2.00 x 102 mL of 0.807 M HCl is mixed with 2.00 10mL of 0.404 M Ba(OH), in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.19°C. For the process H*(aq) + OH(aq) + H2O(1) the heat of neutralization is --56.2 kJ/mol. What is the final temperature of the mixed solution?
Enter your answer in the provided box. A quantity of 2.00 x 102 mL of 0.477 M HCl is mixed with 2.00 x 102mL of 0.239 M Ba(OH), in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.45°C. For the process below, the heat of neutralization is -56.2 kJ/mol. What is the final temperature of the mixed solutions? H(aq) + OH(aq) H20(1).
10. A quantity of 2.00 x 102 mL of 0.862 M HCl (mw: 36.46 g/mol) is mixed with 2.00 x 102 mL of 0.431 M Ba(OH)2 (mw: 171.34 g/mol) in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.48 °C. Given, H+(aq) + OH-(aq) + H2O(1) AH° = -56.2 kſ/mol what is the final temperature (°C) of the mixed solution? Assume the solution mixture has a density of...
A quantity of 8.00 102 mL of 0.600 M HNO3 is mixed with 8.00 102 mL of 0.300 M Ba(OH2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNOs reacts with 0.500 mol Ba(OH)2 is-56.2 kJ/mol Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and·184 J/g·? respectively). What is the final...
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC, the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH" (aq) - H20 (1) is -56.2...
help
2. A quantity of 300 mL of 0.8 M HCl is mixed with 300 mL of 0.4 M Ba(OH)2 in a constant- pressure calorimeter having a heat capacity of 415 J/°C. The initial temperature of both solutions is the same at 22.0°C. Given that the specific heat of the solution is 4.184 J/gºC. the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH(aq) → H20 (1) is -56.2...
Please help
2. Two solutions namely, 500 mL of 0.50 M HCl and 500 mL of 0.50 M NaOH at the same temperature of 21.6 °C are mixed in a constant-pressure calorimeter. The heat capacity of the calorimeter was 450 J/oC. Given that the specific heat of the solution is 4.184 J/g°C, the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H* (aq) + OH (aq) -- H2O (1) is -56.2 kJ,...
A quantity of 12.0 mL of 6.00 M HBr is mixed with 12.0 mL of 6.00 M NaOH in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 21.30°C. The heat of neutralization when 1.00 mol of HBr reacts with 1.00 mol NaOH is -56.1 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water (1,00 g/mL and 4.184 °C. respectively). What is the final...
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