A 50.0 mL of 0.700 M copper (II) sulfate solution is added to a 50.00 mL of 1.00 M sodium hyroxide solution in a coffee cup calorimeter. The initial temperature of the two solutions is 22.5 °C and the highest temperature reached in the calorimeter after mixing is 25.7 °C. Assume that no heat is transferred to the calorimeter or the surroundings and that the heat capacity of the solutions is 4.18 J/g °C. Assume that density of each solution is 1.00 g/mL. Calculate the molar enthalpy change, in kJ/mol, for the precipitation reaction: CuSO4 (aq) +2 NaOH(aq) -----> Cu(OH)2 (s) + Na2SO4 (aq)

A 50.0 mL of 0.700 M copper (II) sulfate solution is added to a 50.00 mL of 1.00 M sodium hyroxide solution in a coffee cup calorimeter. The initial temperature of the two solutions is 22.5 °C and the highest temperature reached in the calorimeter after mixing is 25.7 °C. Assume that no heat is transferred to the calorimeter or the surroundings and that the heat capacity of the solutions is 4.18 J/g °C. Assume that density of each solution is 1.00 g/mL. Calculate the molar enthalpy change, in kJ/mol, for the precipitation reaction: CuSO4 (aq) +2 NaOH(aq) -----> Cu(OH)2 (s) + Na2SO4 (aq)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 104AE

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A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
Microwave ovens convert radiation to energy. A microwave oven uses radiation with a wavelength of 12.5 cm. Assuming that all the energy from the radiation is converted to heat without loss, how many moles of photons are required to raise the temperature of a cup of water (350.0 g, specific heat =4.18J/gC) from 23.0C to 99.0C?
Nitrogen gas is confined in a cylinder with a movable piston under a constant pressure of 9.95 104 Pa. When 695 J of energy in the form of heat is transferred from the gas to the surroundings, its volume decreases by 1.88 L. What is the change in internal energy of the gas?
9.50 When a 13.0-g sample of NaOH(s) dissolves in 400.0 mL of water in a coffee cup calorimeter, the temperature of the water changes from 22.6°C to 30.7C Assuming that the specific heat capacity of the solution is the same as for water, calculate (a) the heat transfer from system to surroundings and (b) H for the reaction NaOH(s)Na+(aq)+OH(aq)
A sample of 0.562 g of carbon is burned in oxygen in a bomb calorimeter, producing carbon dioxide. Assume both the reactants and products are under standard state conditions, and that the heat released is directly proportional to the enthalpy of combustion of graphite. The temperature of the calorimeter increases from 26.74 C to 27.93 C. What is the heat capacity of the calorimeter and its contents?
When 1.0 g of fructose, C6H12O6(s), a sugar commonly found in fruits, is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by 1.58 C. If the heat capacity of the calorimeter and its contents is 9.90 kJ/C, what is q for this combustion?
The addition of 3.15 g of Ba(OH)28H2O to a solution of 1.52 g of NH4SCN in loo g of water in a calorimeter caused the temperature to fall by 3.1 C. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation: Ba(OH)28H2O(s)+2NH4SCN(aq)Ba(SCN)2(aq)+2NH3(aq)+10H2O(l)
What is the difference between the enthalpy of reaction and the enthalpy of formation? For what chemical reaction(s) are the two quantities the same?
A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00C to 33.73C. If the heat capacity of the calorimeter and contents was 9.63 kJ/C, what is the value of q for burning 1.00 mol of ethanol at constant volume and 25.00C? The reaction is C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) Is q equal to U or H?
In a coffee-cup calorimeter, 150.0 mL of 0.50 M HCI is added to 50.0 mL of 1.00 M NaOH to make 200.0 g solution at an initial temperature of 48.2C. If the enthalpy of neutralization for the reaction between a strong acid and a strong base is 56 kJ/mol, calculate the final temperature of the calorimeter contents. Assume the specific heat capacity of the solution is 4.184 J/g C and assume no heat Joss to the surroundings.
Explain why absolute enthalpies and energies cannot be measured, and only changes can be determined.

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