An ideal gas (the system) starts in state 1 and undergoes an irreversible expans

Question

An ideal gas (the system) starts in state 1 and undergoes an irreversible expansion to state 2. It then returns to state 1 via a reversible compression. Which of the following is true for this cycle? delta E_surr > 0 delta S_surr > 0 delta S_sys > 0 delta E_univ > 0 -T delta S_univ = 0 The standard enthalpy of formation of C(s)_diamond is 2 kJ/mol. If a system consisting of 1 mol C(s)_diamond were to turn into C(s)_graphite at constant pressure, what would the heat flow for the system be? Would this reaction be endothermic or exothermic? q = -2 kJ; endothermic q = -2 kJ; exothermic q = 2 kJ; endothermic q = 2 kJ; exothermic q = 0; neither endothermic nor exothermic Which of the following must always be true for a reaction at standard state that has delta G degree

Explanation / Answer

14) B

13) B

120 C

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