The above reaction was performed again, but this time in a constant-pressure calorimeter attached to a frictionless piston. Over the course of the process, the total volume of the gaseous contents of the calorimeter decreased by 100.4 mL. If the pressure outside of the piston was 1.000 atm, determine AHou for this process in kJ. Recall that 101.325 J =1 L atm.

The above reaction was performed again, but this time in a constant-pressure calorimeter attached to a frictionless piston. Over the course of the process, the total volume of the gaseous contents of the calorimeter decreased by 100.4 mL. If the pressure outside of the piston was 1.000 atm, determine AHou for this process in kJ. Recall that 101.325 J =1 L atm.

Chemistry

10th Edition

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 24.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 24.0 L. -23.0 W = Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 1.50 atm to a volume of 16.0 L. 2. From the end point of step 1, let the gas expand to 24.0 L against a constant external pressure of 1.00 atm. W = J J
One day while camping, a student used a propane stove to boil some water. The student heated 5.00 L of water from 15.6°C to 98.5°C. The molar enthalpy of combustion of propane is -2043.9 kJ/mol and heating the water required 1.38 mol of propane. Determine the efficiency of the propane camp stove if the heat released from the stove was used to heat the water. 62.4 % 38.4% D162 % 61.6%
Calculate the work, w, done in kJ when a gas contracts from 55 L to 25 L against a constant external pressure of 1.5 atm. 1 L ∙ atm = 101 J
Find the work energy, w, gained or lost by the system when a sample of gas expands from 10 L to 30 L against a constant external pressure of 2.0 atm. [1L· atm = 101 J] -1.01 KJ -3.02 KJ -2.02 KJ 4.04 KJ
Measurements show that the energy of a mixture of gaseous reactants decreases by 174. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -131. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. O exothermic Is the reaction exothermic or endothermic? O endothermic
None
The experimental enthalpy of decomposition of H2O2 was determined using another coffee-cup calorimetry. A sample of H202 solution was placed in the calorimeter and the initial temperature of H202 solution and the calorimeter was measured. Then, KI solution was added to the solution to catalyze the decomposition of H202 to H20. This resulted to an increase of 16.9°C in the temperature. Determine the experimental enthalpy of decomposition per mole of H2O2 given the following additional information. Express your answer in kJ/mol and in 2 decimalplaces. moles H202: 0.018 mol Ccal: 54.56 J/°C mass of the solution (mainly water): 33.9 g C, of water: 4.184 J/g°C
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 24.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 24.0 L. w = J Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 1.50 atm to a volume of 16.0 L. 2. From the end point of step 1, let the gas expand to 24.0 L against a constant external pressure of 1.00 atm. w = J
00 IN L OUniversity Science Book: presented by Macmillan Learning Stry 4th Edition McQuarrie Rock Gallogly Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 18.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 18.0 L. Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 1.80 atm to a volume of 10.0 L. 2. From the end point of step 1, let the gas expand to 18.0 L against a constant external pressure of 1.00 atm. = M Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher. University Science Books MacBook Pro Q Search or enter website name { [ 7. $4 P. 5. 4. U E. K. H. B. gE
Consider a gas cylinder containing 0.250 moles of an ideal gas in a volume of 6.00 L. The cylinder is surrounded by a constant temperature bath at 292.0 K. With an external pressure of 3.00 atm, the cylinder is compressed to 2.00 L. Calculate the work of the gas for this compression process, in J (Recall that there are 101.325 J/L•atm)
A 25.0 mL portion of dilute HCl (aq) is combined with a 25.0 mL portion of dilute NaOH in a coffee-cup calorimeter. Both solutions are initially at a temperature of 23.3 ºC. The reaction produces enough heat to raise the final temperature of the 50.0 mL of liquid in the calorimeter to 25.3 ºC . What is qrxn in J? Assume the density of the reaction mixture is 1.0 g/mL and the specific heat of the solution is 4.184 J/g· ºC