08:42Thermochemical Equations and Using the energy term (heat of reaction) in mole-mass problem solvingCrash Chemistry Academy523views
Multiple ChoiceNitromethane (CH3NO2), sometimes used as a fuel for drag racing, burns according to the following reaction: 4 CH3NO2 (l) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (g) + 4 NO2 (g) ∆Hº = – 2441.6 kJHow much heat is released by burning 125.0 g of nitromethane (MW:61.044 g/mol)? 2017views4rank1comments
Multiple ChoiceConsider the following reaction: 2 C6H6 (l) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (g) ∆Hº = – 6278 kJWhat volume of benzene (C6H6, d = 0.880 g/mL, molar mass = 78.11 g/mol) is necessary to evolve 5.19 x 109 kJ of heat? 970views
Multiple ChoiceThe creation of liquid methanol is accomplished by the hydrogenation of carbon monoxide: CO (g) + 2 H2 (g) → CH3OH (l) ∆Hº = – 128.1 kJHow much heat (in kJ) is released when 125.0 g CO reacts with 2.32 x 102 g H2?2376views4rank1comments
Multiple ChoiceConsider two identical iron nails: One nail is heated to 95℃, the other is cooled to 15℃. The two nails are placed in a coffee cup calorimeter and the system is allowed to come to thermal equilibrium. What is the final temperature of the two nails?369views
Open QuestionWhich answer best describes the transfer of heat that occurs when 1.50 mol of H2 reacts?240views
Open QuestionConsider the thermochemical equation for the combustion of acetone (C3H6O), the main ingredient in nail polish remover: C3H6O(l) + 4 O2(g) → 3 CO2(g) + 3 H2O(g) ΔH°rxn = -1790 kJ. If a bottle of nail polish remover contains 177 mL of acetone, how much heat is released by its complete combustion? The density of acetone is 0.788 g/mL.
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