The thermochemical equation for the combustion of methanol is CH3OH (g)  +  3/2 O2(g)  →  CO2(g)  +  2 H2O(l)       ΔH = -764 kJ mol-1  How many kJ of heat are produced when 5.00 g of methanol reacts with excess oxygen gas as shown in the equation?   (molar mass of methanol, CH3OH:  32.05 g mol-1)   a. 4.77 kJ b. 153 kJ c. 764 kJ d. 3820 kJ e. 119 kJ

Consider the reaction of hydrogen with sulfur to form hydrogen sulfide: 8H₂ (g) + Sg (s) → 8H₂S(g), which has an enthalpy of reaction of -20.15 kJ/mol. If 150 g of sulfur are reacted with an excess of hydrogen, how much heat is produced (kJ)?

How many moles of H2 are required to produce -2501 KJ of heat in the following reaction?       Heat of Formation = -91.8 KJ/mol    N2(g) + 3 H2(g) --> 2NH3(g)

Calculate how much heat is released when 200 grams of NH3 is mixed with 450 grams of O2.4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g ) ?H= - 1530 kJ

61. Consider the thermochemical equation for the combustion of acetone (CH,O), the main ingredient in nail polish remover: C;H,O(l) + 4 O,(g) 3 CO2(g) + 3 H,O(g) A,H° = -1790 kJ mol 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.

The complete combustion of propane, C 3H 8(g), is represented by the equation: C 3H 8(g) + 5 O 2(g) → 3 CO 2(g) + 4 H 2O(l) Δ H° = -2220 kJ How much heat is evolved in the complete combustion of 2.50 g C 3H 8(g)?

Consider the following reaction: 2 H2(g) + O2(g)  2 H2O(l) Answer the following questions: (a) How much heat is evolved when 1.249×101 moles of H2O(l) is produced from the combustion of H2(g).Answer to 4 sig figs. (b) How much heat is evolved when 1.310×101 g of H2(g) is burned in excess oxygen.Answer to 4 sig figs. (c) How much heat is evolved when 1.736×102 moles of H2(g) is burned in excess oxygen.Answer to 4 sig figs.

Here's a formula for the combustion of ethane: 2 C,H, (g) + 7 O, (g) → 6 H,O (g) + 4 CO2 (g) AH = -5318 kJ/mol a.) How many grams of ethane do I need to burn to generate 50,000 kJ of heat?

When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released, as shown in the combustion reaction. CH, OH(g) + O₂(g) → CO₂(g) + 2H₂O(1) AH = -764 kJ Based on the balanced thermochemical reaction, how much heat is produced when 25.7 g of methanol reacts with 39.9 g of oxygen? heat: Which reactant is limiting? methanol oxygen kJ

Consider these reactions: Reaction 1: H₂(g) + Cl₂ (g) 2HCl(g) AH-184.6 kJ Reaction 2: 20F2(g) O₂(g) + 2 F₂ (g) AH = -49.4 kJ Reaction 3: N₂(g) + 2O₂(g) · 2NO₂(g) AH = +66.4 kJ