The work done on the system (w) = -P.V = -P(V2 - V1) = -7 atm * (1 - 5.5) L = 31.5 L.atm = 3189.9 J or 3.19 kJ
According to the definition of enthalpy change, H = U + (-w), i.e. 11.5 kJ = U + (-3.19), i.e. U = 14.7 kJ
A system absorbs 11.5 KJ of heat while it is compressed from 5.5 L to 1.0...
A system absorbs 21.6 kJ of heat while performing 6.9 kJ of work on the surroundings. If the initial internal energy, E, is 61.2 kJ, what is the final value of E? [ NOTE: Remember “∆” = final – initial]
1.) A system absorbs 1.56E+2 kJ of heat and the surroundings do 1.107E+2 kJ of work on the system. What is the change in internal energy (in kJ) (ΔU) of the system? 2.) A sample of gas in a cylinder is provided with 6.221E+2 kJ of heat. This causes a piston to then compresses the gas by doing 4.343E+2 kJ of work to the gas. What is the change in internal energy of the gas during this compression? 3.)A gas...
1)A gas is compressed at a constant pressure of 0.800 atm from 8.00 L to 1.00 L. In the process, 410 J of energy leaves the gas by heat. (a) What is the work done on the gas? J (b) What is the change in its internal energy? J 2) A gas increases in pressure from 2.00 atm to 6.00 atm at a constant volume of 1.00 m3 and then expands at constant pressure to a volume of 3.00 m3...
A system absorbs 196 kJ of heat and the surroundings do 117 kJ of work on the system. Calculate the change in internal energy of the system.
A system absorbs 187 kJ of heat and the surroundings do 120 kJ of work on the system. What is the change in internal energy of the system? Express the internal energy in kilojoules to three significant figures.
HQ11.13 Homework Unanswered The air in an inflated balloon (the system) absorbs 2 kJ of heat from its proximity to a fire. The balloon expands and does 85 kJ of work. What is the change in internal energy (in kJ) (AU) for the system? Numeric Answer:
Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L • atm)
Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L • atm)
Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L • atm)
Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L • atm)