Write the thermochemical equation for the following reaction that occur at constant pressure. 1.) Combustion of Hexane, C6H12, to carbon dioxide gas and water, releases 3923.9 kJ of heat.

What quantity of heat (in kJ) will be released if 0.2921 mol of NH3 are mixed with 0.200 mol of O₂ in the following chemical reaction? 4 NH3(g) + O₂ (g) → 2 N₂H4 (g) + 2 H₂O (g) AH° = -286 kJ/mol

Question 18 of 39 Submit In the following reaction, how many moles of CH3OH are required to give off 5576 kJ of heat? 2 CH,OH (I) + 3 O2 (g) → 2 CO2 (g) + 4 H¿O(g) AH° = -1280. kJ mol 1 2 3 4 C 7 +/- x 10 0 LO 00

If 176.3 kilojoules of heat were released when iron, Fe, was burned to form Fe2O3(s) at standard state conditions, what mass of iron (in g) was originally present

How much heat is rel;eased to the surroundings when 5.00 g of CO2 is produced according to the following thermochemical equation? C3H8 + 5 O2 --> 3 CO2 + 4 H, AHn = -2220 kJ/mol %3D Note: the molar mass of CO2 is 44.0 g/mol 757 kJ O252 kJ 740 kJ 84.1 kJ

Octane (C8H18) is a component of gasoline that burns according to the following equation:  C8H18 (l) + 25/2 O2 (g) ------> 8 CO2 (g) + 9 H2O (g) ΔHorxn = - 5074.1 kJ What mass of octane (in g) is required to produce 5830 kJ of heat?

Calculate the heat necessary to increase temperature of a) 100. g of water b) 2.00 mol H2O(l) from 20 ℃ to 100 ℃.

What quantity of heat (in kJ) will be released if 0.1673 mol of NH³ are mixed with 0.200 mol of O: in the following chemical reaction? 4 NH (g) + O: (g) → 2 N₂H4 (g) + 2 H₂O (g) AH = -286 kJ/mol

Constant is 4.184