Homework Answers
ANSWER:
The heat change = mass X heat capacity X Temperature difference.
mass = mass of H2O2 + Mass of Fe(NO3)3
Mass of H2O2 = No. of moles X molar mass
Mass of H2O2 = Molarity X volume in L X molar mass ( because No. of moles = Molarity X volume)
Mass of H2O2 = 0.88 X 0.05 X 34 = 1.496g
Similarly mass of Fe(NO3)3 = 0.5 X 0.01 X 241.86 = 1.209g
Total mass = 2.705g
The heat change =2.705g X 5.0J/Co X 7.57 = 102J
A 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined...
A 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined and a temperature change of 6.61 was observed. The specific heat of water is 4.18 J/(g * ∘C) Calculate the total heat change (in kilojoules) for the calorimeter. Record your answer with the proper significant figures and include the correct sign if needed. Assume the density and specific heat of the solution are the same as that of water.
If 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined...
If 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined and a temperature change of 8.03°C was observed, The specific heat of water is 4.18 J/(g * ∘C) Calculate the enthalpy of decomposition of hydrogen peroxide (ΔH) determined from the experimental data. Record your answer with the proper significant figures and include the correct sign if needed. Assume the density and specific heat of the solution are the same as that of water.
measurements show that unknown compound X has t A 50.0 mL of 0.88 M H2O2 and...
measurements show that unknown compound X has t
A 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined and a temperature change of 7.57 was observed. The specific heat of water is 4.18 J/g * .C). Calculate the total heat change (in kilojoules) for the calorimeter. Record your answer with the proper significant figures and include the correct sign if needed. Assume the density and specific heat of the solution are the same as...
A 50 mL of 0.88 M H2O2 and 10 mL of 0.50 M Fe(NO3)3 were combined...
A 50 mL of 0.88 M H2O2 and 10 mL of 0.50 M Fe(NO3)3 were combined and a temperature change of 8.11 was observed. The specific heat of water is 4.18 J/(g * ∘C) Calculate the heat of reaction (in kilojoules). Record your answer with the proper significant figures and include the correct sign if needed.
1. 50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°C...
1. 50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°C in a calorimeter also at 23.2°C. The final temperature was 33.1°C. Assuming that neither the density of water nor its specific heat capacity change with temperature, calculate the total heat capacity of the calorimeter. (density of water = 1.00 g mlº', specific heat capacity=4.18 J g?K=) 2. When 5.00 g of NaOH(s) are added to 100 g of water (using the same calorimeter as...
A 100.0 mL of 0.50 M HCl at is reacted with 125.0mL of 0.50 M NaOH...
A 100.0 mL of 0.50 M HCl at is reacted with 125.0mL of 0.50 M NaOH in a calorimeter whose heat capacity is 500 J/C. What will the maximum temperature reached by the resulting solution if the initial temperature for the solution is 20.0°C? (Assume that the specific heat of the final solution is 4.18 J/g·°C, and that the density of the final solution is that of water.) The enthalpy change of HCl acid is neutralized by NaOH is –56...
If 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined...
If 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined and a temperature change of -6.61°C was observed, The specific heat of water is 4.18 J/(g * ∘C) Calculate the heat of reaction (in kilojoules). Record your answer with the proper significant figures and include the correct sign if needed.
50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°C in...
50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°C in a calorimeter also at 23.2°C. The final temperature was 33.1°C. Assuming that neither the density of water nor its specific heat capacity change with temperature, calculate the total heat capacity of the calorimeter. (density of water = 1.00 g mL"', specific heat capacity= 4.18 J g'K:')
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,...
Exam time remaining: 146 minute A 50.0 mL of 0.88 M H2O2 and 10.0 mL of...
Exam time remaining: 146 minute A 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined and a temperature change of 7.47 was observed. The specific heat of water is 4.18 J/g.c) Calculate the heat of reaction (in kilojoulos). Record your answer with the proper significant figures and include the correct signif needed. Assume the density and specific heat of the solution are the same as that of water. Buck Next
measurements show that unknown compound X has t
A 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined and a temperature change of 7.57 was observed. The specific heat of water is 4.18 J/g * .C). Calculate the total heat change (in kilojoules) for the calorimeter. Record your answer with the proper significant figures and include the correct sign if needed. Assume the density and specific heat of the solution are the same as...
1. 50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°C in a calorimeter also at 23.2°C. The final temperature was 33.1°C. Assuming that neither the density of water nor its specific heat capacity change with temperature, calculate the total heat capacity of the calorimeter. (density of water = 1.00 g mlº', specific heat capacity=4.18 J g?K=) 2. When 5.00 g of NaOH(s) are added to 100 g of water (using the same calorimeter as...
50 mL of water at 51.9°C were mixed with 50 mL of water at 23.2°C in a calorimeter also at 23.2°C. The final temperature was 33.1°C. Assuming that neither the density of water nor its specific heat capacity change with temperature, calculate the total heat capacity of the calorimeter. (density of water = 1.00 g mL"', specific heat capacity= 4.18 J g'K:')
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,...
Exam time remaining: 146 minute A 50.0 mL of 0.88 M H2O2 and 10.0 mL of 0.50 M Fe(NO3)3 were combined and a temperature change of 7.47 was observed. The specific heat of water is 4.18 J/g.c) Calculate the heat of reaction (in kilojoulos). Record your answer with the proper significant figures and include the correct signif needed. Assume the density and specific heat of the solution are the same as that of water. Buck Next
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