first law of thermodynamics states that
(heat in - heat out ) + (work in -work out ) =change in internal energy of the system
hence 0-25000 + 1.5*101.3 (12-6)-0 =chage in internal energy
hence change in internal energy =24.08 KJ=24.1 KJ
here change in internal energy = final internal energy - initial internal energy
hence initial internal energy-final internal energy= -24.1 kJ
Calculate the change in internal energy (?E) for a system that is giving off 25.0 kJ of heat and is changing from 12.00...
Calculate the change in internal energy (?E) 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) 13) ______ A) +25.9 kJ B) 937 kJ C) -24.1 kJ D) -16.0 kJ E) -25.9 kJ
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)
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