Author Question: 8.000 moles of H2(g) reacts with 4.000 mol of O2(g) to form 8.000 mol of H2O(l) at 25 C and a ... (Read 114 times)

DyllonKazuo · **on:** Nov 18, 2019

Question 1

For a particular process that is carried out at constant pressure, q = 145 kJ and w = -35 kJ. Therefore,
◦ ΔU = 180 kJ and ΔH = 145 kJ.
◦ ΔU = 110 kJ and ΔH = 145 kJ.
◦ ΔU = 145 kJ and ΔH = 110 kJ.
◦ ΔU = 145 kJ and ΔH = 180 kJ.

Question 2

8.000 moles of H2(g) reacts with 4.000 mol of O2(g) to form 8.000 mol of H2O(l) at 25 °C and a constant pressure of 1.0133 bar. If 546.4 kJ of heat are released during this reaction, and PΔV is equal to -29.60 kJ, then
◦ ΔH° = -546.4 kJ and ΔU° = -516.8 kJ.
◦ ΔH° = +546.4 kJ and ΔU° = +576.06 kJ.
◦ ΔH° = -546.4 kJ and ΔU° = -576.0 kJ.
◦ ΔH° = +546.4 kJ and ΔU° = +516.8 kJ.

batool · **Reply #1 on:** Nov 18, 2019

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