Energy change is the sum of heat and work: ΔE = q + w. Work is calculated by: w = -PΔV
What is the change in energy (in joules) if a reaction absorbs 72.8 J of heat and increases in volume from 0.250L to 0.750L at a constant pressure of 1.168 atm? Please include the correct sign with your numerical result.
(Note: Make sure your units are consistent when combining energy terms. The conversion factor you need is: 1 L·atm = 101.3 J)
I need help setting up this problem and identifying the variables Energy change is the sum of heat and work: ΔE = q + w. Work is calculated by: w = -PΔV What is the change in energy (in joules) if a reaction loses 215 J of heat and decreases in volume from 0.650 L to 0.225 L at a constant pressure of 3.17 atm? Please include the correct sign with your numerical result.
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)
400 J of heat is added to a system. If the change in internal energy of the system was 850 J, how much work was done on by the system? the inside a container absorbs 250 J of hea while 125 J of work is done on it and then does 70 J of its own work, by how much does the internal energy of the gas increase? 7.500 joules of heat is added to a system while it also...
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 (?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
What is the change in energy (in joules) if a reaction loses 399 J of heat and decreases in volume from 0.650 L to 0.225 L at a constant pressure of 4.65 atm? Please include the correct sign with your numerical result.
What is the overall change in internal energy for System A after both of the following processes have occurred? Process 1: System A absorbs 10 kJ of heat from the surroundings and does 8 kJ of work on its surroundings. Process 2: System A releases 5 kJ of heat into the surroundings and 10000 J of work is done on the system. 2 kJ, ΔE = negative 7 kJ, ΔE = positive 33 kJ, ΔE = negative 9982 J, ΔE...