Reaction

A 2 mole sample of gas expands from a volume of 4 L to 10 L under a constant pressure of 12.5 atm before then dropping to a pressure of 5 atm (while remaining at 10 L). 2 moles of gas expands from a volume of 4L to 10 L under a constant temperature (300K). Which situation requires more work? Why?

When one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2 and liquid water are formed. The reaction absorbs 90.1 KJ of heat.  a. Write a balanced thermochemical equation for the reaction. b. Calculate ∆H°f for calcium cyanamide.

4. Two solutions, initially at 24.60°C, are mixed in a coffee cup calorimeter (Ccal = 15.5 J/°C). When a 100.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.200 M NaCl solution, the temperature in the calorimeter rises to 25.30°C. Determine the AH°rxn for the reaction. Dsol'n = 1.00 g/mL. Csol'n = 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

Which of the following best defines molar heat capacity. a. The quantity of heat required to raise the temperature of 1 mole of a substance by 1K   b. The quantity of heat required to lower the temperature of 1 liter of a substance by 1°C   c. The quantity of heat required to raise the temperature of 1 gram of a substance by 1°C   d. The quantity of heat required to raise the temperature of 1 gram of a substance by 1°F

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