Question

Which answer best describes the transfer of heat that occurs when 1.71 mol of h2 reacts with 0.814 mol of o2?

Answer 1

The reaction between H2 and O2 to form water can be shown as below:

2H2 (g) + O2 (g) → 2H2O (l)

This is an exothermic reaction where the enthalpy change (heat released) = -484 kJ

Here we have 1.71 moles of H2 reacting with 0.814 moles of O2. Since moles of O2 < moles of H2, the former will be the limiting reagent.

Since the heat transferred by 1 mole of O2 is -484 kJ,

The heat corresponding to 0.814 moles of O2 would be

= 0.814 moles O2 * -484 kJ/ 1 mole O2 = -393.97 kJ

Ans: Heat transfer = -394 kJ

Answer 2

Heat is released when hydrogen and oxygen atom combine with each other.

What is exothermic reaction?

Exothermic reactions are those type of reaction that release heat and light to their surroundings. When two atoms combine to form a bond, some heat is always released which is called bond formation energy so we can conclude that heat is released when hydrogen and oxygen atom combine with each other.

Learn more about heat here: https://brainly.com/question/13439286