If all of the energy from burning 294.0 g of propane (ΔΔHcomb,C3H8 = –2220 kJ/mol) is used to heat water, how many liters of water can be heated from 20.0°C to 100.0°C? (Assume that the density of water is 1.00 g/mL)

CH4 + 202 → CO₂ + 2H₂O AH-890kJ/mol How much heat is released when 2.7 g of methane gas is burned in a constant pressure system?

In the following reaction, how much heat (in kJ) is released when 5.63 moles of CH₄ are burned? CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ∆H° = -802 kJ/mol

In the following reaction, how much heat is generated when 2.53 moles of CH₄ are burned? CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ∆H° = -802 kJ/mol

How much energy in kJ is released in burning 1.63 mL of gasoline (assuming that all of it is octane with a density of 0.692 g/mL and a molar mass of 114.23 g/mol)   The equation for the combustion reaction is C8H18(ℓ) + 25/2O2(g) → 8CO2(g) + 9H2O(ℓ)   ΔHf° kJ/mol C8H18(ℓ): -250.3 O2(g): 0 CO2(g): -393.5 H2O(ℓ): -285.8   Round your answer to 2 decimal places.

In the following reaction, what is the quantity of heat (in kJ) released when 4.93 moles of CH₄ are burned? CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ∆H° = -802 kJ/mol

2. The decomposition of ammonia gas into nitrogen gas and hydrogen gas is endothermic:   2 NH3 (g) → N2 (g) + 3 H2 (g)     ΔH = 92 kJ/mol   If 762 mL of hydrogen gas, measured at 325°C and 792 mmHg, is formed in the reaction above, how much heat will be absorbed?

Charcoal is primarily carbon. Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 5.00 * 102 kJ of heat.C(s) + O2(g) ------->CO2(g) ∆H° rxn = -393.5 k

Ethyl alcohol, C2H5OH, has a specific heat of 2.40 ?? °?. Which of the following statements best describes what this means? a) It takes 1 joule of energy to increase the temperature of 1 gram of ethyl alcohol by 2.40 °C. b) It takes 1 joule of energy to increase the temperature of 2.40 grams of ethyl alcohol by 1 °C. c) It takes 2.40 joules of energy to increase the temperature of 1 gram of ethyl alcohol by 1 °C. d) It takes 2.40 joules of energy to increase the temperature of 2.40 grams of ethyl alcohol by 1 °C