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17 Nov 2019
I need help with 4-6. Can you please show work
Consider the reaction: CH_4 (g) + 2O_2 (g) rightarrow CO_2 (g) + 2H_2O (l) Delta H = -890 kJ How many grams of methane (CH_4) must be burned to produce (release) 267 kJ of heat? When 0.514 g biphenyl (C_12H_10) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8 degree C to 29.4 degree C. The heat capacity of the calorimeter is 5.86 kJ/degree C. Calculate: q_rxn per mole of biphenyl for the combustion process q_rxn per gram of biphenyl for the combustion process Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s) + 2HCl(aq) rightarrow ZnCl_2 (aq) + H_2 (g) When 0.103 g of zinc is reacted with 50.0 g of HCl solution in a coffee-cup calorimeter, the temperature rose from 22.5 degree C to 23.7 degree C. Assume that the specific heat of the solution is the same as that of pure water, 4.18 J/g degree C. Calculate: Delta H_rxn per mol zinc for this reaction Delta H_rxn per gram of zinc for this reaction
I need help with 4-6. Can you please show work
Consider the reaction: CH_4 (g) + 2O_2 (g) rightarrow CO_2 (g) + 2H_2O (l) Delta H = -890 kJ How many grams of methane (CH_4) must be burned to produce (release) 267 kJ of heat? When 0.514 g biphenyl (C_12H_10) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8 degree C to 29.4 degree C. The heat capacity of the calorimeter is 5.86 kJ/degree C. Calculate: q_rxn per mole of biphenyl for the combustion process q_rxn per gram of biphenyl for the combustion process Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s) + 2HCl(aq) rightarrow ZnCl_2 (aq) + H_2 (g) When 0.103 g of zinc is reacted with 50.0 g of HCl solution in a coffee-cup calorimeter, the temperature rose from 22.5 degree C to 23.7 degree C. Assume that the specific heat of the solution is the same as that of pure water, 4.18 J/g degree C. Calculate: Delta H_rxn per mol zinc for this reaction Delta H_rxn per gram of zinc for this reaction
Casey DurganLv2
29 Jan 2019