Author Question: When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of H2O(l) at 25C and a ... (Read 118 times)

cool · **on:** Feb 15, 2020

Question 1

For an explosion in an open vessel, one would expect
◦ ΔH to be positive and ΔE to be less than ΔH.
◦ ΔH to be positive and ΔE to be greater than ΔH.
◦ ΔH to be negative and ΔE to be greater than ΔH.
◦ ΔH to be negative and ΔE to be less than ΔH.

Question 2

When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 1366 kJ of heat are released during this reaction, and PΔV is equal to -74.00 kJ, then
◦ ΔH° = -1366 kJ and ΔE° = -1440 kJ.
◦ ΔH° = +1366 kJ and ΔE° = +1440 kJ.
◦ ΔH° = -1366 kJ and ΔE° = -1292 kJ.
◦ ΔH° = +1366 kJ and ΔE° = +1292 kJ.

amit · **Reply #1 on:** Feb 15, 2020

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