Calculate w and ΔE when 1 mole of a liquid is vaporized at its boiling point (80oC) and 1.00 atm pressure. ΔHvap for the liquid is 30.7 kJ mol21 at 80.oC.
Answer to relevant QuestionsGiven the following data: Calculate ΔH for the reaction On the basis of enthalpy change, is this a useful reaction for the synthesis of ammonia? Given the following data: Ca(s) + 2C(graphite) → CaC2(s) ΔH = –62.8 kJ Ca(s) + ½ O2(g) → CaO(s) ΔH = –635.5 kJ CaO(s) + H2O(l) → Ca(OH)2(aq) ΔH = –653.1 kJ C2H2(g) + 5/2 O2(g) → 2CO2(g) 1 H2O(l) ΔH = ...A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 72 J of heat while 35 J of work is done on it. Step 2: The system absorbs 35 J of heat while performing 72 J of work. Calculate ...At 298 K, the standard enthalpies of formation for C2H2(g) and C6H6(l) are 227 kJ/ mol and 49 kJ/ mol, respectively. a. Calculate ΔHo for C6H6(l) → 3C2H2(g) b. Both acetylene (C2H2) and benzene (C6H6) can be used as ...Methanol (CH3OH) has also been proposed as an alter-native fuel. Calculate the standard enthalpy of combustion per gram of liquid methanol, and compare this answer to that for ethanol in Exercise 80.
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