CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)Δ?=−764 kJ   How much methanol, in grams, must be burned to produce 657 kJ of heat? mass:

You mix 125 mL of 0.210 M CsOH with 50.0 mL of 0.525 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 21.30 °C before mixing to 23.73 °C after the reaction. CsOH(aq) + HF (aq) → CsF(aq) + H₂O(l) What is the enthalpy of reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g. K. Enthalpy of reaction = kJ/mol

Calculate the energy required to heat 202.0mg of cyclohexane from 18.4°C to 38.8°C . Assume the specific heat capacity of cyclohexane under these conditions is 1.85J·g−1K−1 . Be sure your answer has the correct number of significant digits.

Consider the thermochemical equation for the combustion of acetone (C3H₂O), the main ingredient in nail polish remover: C3H6O (1) + 4 O₂ (g) → 3 CO₂ (g) + 3 H₂O (g) ΔΗ° rxn = 1790 kJ If a bottle of nail polish remover contains 222 mL of acetone, what is the magnitude (the value) of heat released by the complete combustion of the acetone in the bottle? The density of acetone is 0.788 g/mL. The molar mass of acetone is 58.08 g/mol. The units are kJ. Do not include units in your answer.