How much energy is needed for the reaction of 1.22 moles of H3BO3 with 5.67 moles of hydrogen

The combustion of propane gas (C3H8; molar mass = 44.09 g/mol) occurs according to the following equation:                  C3H8(g)  +  5O2(g)  -->  3CO2(g)  +  4H2O(g)    Given the following standard molar enthalpy of formation (DHof), how much energy in kilojoules is produced when 1.00 g of propane is completely combusted?               DHof[C3H8] = -103.8 kJ/mol;  DHof[CO2] = -393.5 kJ/mol, and  DHof[H2O(g)] = -241.8 kJ/mol          (A) 2043.9 kJ          (B) 531.5 kJ          (C) 12.1 kJ          (D) 46.4 kJ

of ld 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) - ►H,O(1) endothermic or exothermic? b) In which direction does heat flow? 175

A scientist measures the standard enthalpy change for this reaction to be 296.0 kJ/mol: H₂S(g) + 2 H₂O(l) 3H₂(g) + SO₂(g) Based on this value and the standard formation enthalpies for the other substances, the standard formation enthalpy of H₂S(g) is kJ/mol. Submit Answer Retry Entire Group 1 more group attempt remaining

Propane (C3H8) is the commonly used fuel in our barbeques at home. It is a great fuel because it will release 2220 kJ of energy for every mole that combusts. A. Write the balanced reaction for the combustion of propane. B. When 50.0g of propane cobusts, how much energy is released? C. Is this reaction exothermic or endothermic? Provide evidence.

Given the following information: Cao (s) + H20 (1) -- Ca(OH) 2(s) AHO = -62.5 kJ/ mol How many grams of Cao must react in order to liberate 625 kJ of heat? (The molar mass of CaO is 56 g.)