Question

The lesson is about First Law of Thermodynamic. The problems have answers but i need solutions. PLEASE HELP ME! THANK YOU!

38. Calculate the maximum work that could be obtained if 2.00 mol of an ideal gas, initially at STP, is allowed to expand to 100 L isothermally. Answer-36.0 L-atm 39. If 5.00 mol of an ideal gas is heated at constant pressure from 300 K to 500 K, how much work is done by the expansion of the gas? Answer -8.31 kJ 40. Calculate the change in internal energy of a quantity of gas that absorbs 1000 cal of heat while expanding from 15 L to 25 L at a constant pressure of 4.0 atm. Answer: 31 cal 41. Calculate w, 4. AE, and AH if 1 mol of an ideal gas, initially at 20 °C and 8.0 atm, undergoes an isothermal expansion against a constant pressure of 2.0 atm until the final pressure is 2.0 atm. Answer: -1.8 kJ 42. Calculate the amount of heat required to raise the temperature of 1.00 mol H2 from 300 K to 1200 K at constant pressure. Don't assume that heat capacity is constant. Answer: 26.7 kJ 43. For a certain ideal gas, Cv.m - 3/2 R. If 1 mol of this gas undergoes an adiabatic reversible expansion from STP to a volume of 40.0 L, what is the final temperature? Answer: 185 K 44. An ideal gas, initially at 400 K and 4.00 atm, is allowed to expand reversibly and adiabatically until the temperature has dropped to 300 K. What is the final pressure? (Cv.m - 5/2 R.) Answer: 1.46 atm 45. Calculate the heat required to raise the temperature of 200 g SO, from 300 K to 500 K Assume no dissociation. Answer: 6.95 kcal 46. In an experimental determination of the specific heat of nickel, an 8.78.g piece of the metal was heated in boiling water long enough to be thoroughly heated to the metal's boiling temperature of 99.3°C. Then it was transferred rapidly to 9.54 g of water at 24.2°C. The temperature of the water rose to 31.1°C. Calculate the experimental value of the specific heat of nickel. Answer: 0.110cal/gK

Answer 1

38)

for isothermal process of an ideal gas, the formula for work is given by:

...........(1)

where, W = work done

n = number of moles

R = universal gas constant = 0.0821 (L atm)/ (mol K)

T = temperature

V2 and V1 = volume at state 2 and 1 respectively

P2 and P1 = pressure at state 2 and 1 respectively

first, we have to determine volume at state 1.

note:

as per HOMEWORKLIB RULES, first question of multiple questions has been solved.