A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 JoC-1g-1) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 JoC-1g-1) are heated to 100.0oC. The mixture of hot iron and aluminum is then dropped into 97.3 g of water at 22.0oC. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.
Answer to relevant QuestionsA sample of nickel is heated to 99.8oC and placed in a coffee cup calorimeter containing 150.0 g water at 23.5oC. After the metal cools, the final temperature of metal and water mixture is 25.0oC. If the specific heat ...The heat capacity of a bomb calorimeter was determined by burning 6.79 g of methane (energy of combustion = –802 kJ/ mol CH4) in the bomb. The temperature changed by 10.8oC. a. What is the heat capacity of the bomb? b. A ...Given the following data: C2H2(g) + 5/2 O2(g) → 2CO2(g) + H2O(l) ΔH = –1300. kJ C(s) + O2(g) → CO2(g) ΔH = –394 kJ H2(g) + ½ O2(g) → H2O(l) ΔH = -286 kJ calculate ΔH for the reaction 2C(s) + H2(g) → C2H2(g) Given the definition of the standard enthalpy of formation for a substance, write separate reactions for the formation of NaCl, H2O, C6H12O6, and PbSO4 that have ΔHo values equal to ΔHof for each compound. 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 ...
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