Methanol is used to heat food. The combustion of methanol can be described by the following thermochemical equation: 2CH3OH(I) + 3O2(8) 2CO2(3) + 4H20(g) AH° = -1199 kJ How much methanol, in grams, is needed to release 573 kJ of heat?

According to the reaction below, determine the amount heat (in kJ) that can be generated from the combustion of 1.42 grams of C3H8?   C3H8(g) + 5O2(g) ⟶⟶ 3CO2(g) + 4H2O(g)     Δ?=−2043.2??

It is recommended that the average daily intake of glucose for humans is not to exceed 32.5 g of glucose (C6H12O6). The balanced chemical equation for the combustion of glucose is shown below. C6H12O6(aq) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O (1) AH rxn= -1273.3 kJ/mol How much heat is released when 55.5 g of oxygen are combusted with glucose as shown in the reaction. above? Use the provided Periodic Table for any calculations involving elements. Report your answer to a single decimal place and report proper units with your answer.

Given the following thermochemical equations P4(s) + 6C12(g) 4PCI3(g) AH = -2439 kJ/mol 4PCI5(g) → P4(s) + 10CI 2(g) AH = 3438 kJ/mol find the AH for the reaction below, PCI5(g) → PC|3(g) + Cl2(g) O A) +249.8 kJ/mol O B) +999 kJ/mol O C) -999 kJ/mol O D) -249.8 kJ/mol