Calculate ΔE for the following situations:
q = 6.900 kJ; w = 0.7000 J
q = -545.0 J; w = -335.0 J
Calculate ΔE for the following situations: q = 6.900 kJ; w = 0.7000 J q = -545.0 J; w = -335.0 J
For ammonia, ΔHvap = 23.6 kJ/mol at its boiling point, -33 oC. Calculate the values for ΔS, q, w, and ΔE for the vaporization of ammonia at -33 oC and 1 atmosphere pressure.
Part A Calculate E, if q #: 0763 kJ and w :--840 J Express your answer using two significant figures.
Please show all work and explanations! Calculate ΔE, ΔS, ΔG, Q and W for the vaporization of 3.00 moles of liquid water to form water vapor at 100°C and 1.00 atm pressure. The standard molar enthalpy of vaporization of water is 40.67 kJ/mol. The density of liquid water at 100°C is 0.958 g/cm3 . Assume that the water vapor is an ideal gas, but be careful – the initial state is liquid water, so this is not simply an ideal...
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...
Calculate w and ΔE when 2 mol of liquid ZnC4H10 is vaporized at 265 K and 760 mm Hg. The ΔH vaporization is 39.9 kJ/mol at 265 K.
What are ΔE, q, w and ΔH for the evaporation of 18.3 g of Br2(l) at 298 K and 1 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)
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)