For a reaction with ΔH = -120 kJ, how much heat is absorbed when 0.25 moles of r

For a reaction with ΔH = -120 kJ, how much heat is absorbed when 0.25 moles of reactants are converted?

For a reaction with ΔH = -120 kJ, how much heat is absorbed when 0.25 moles of reactants are converted?

Step 1: Understand that ΔH represents the change in enthalpy (heat) for the reaction. Here, ΔH = -120 kJ means that the reaction releases 120 kJ of heat.
Step 2: Identify how many moles of reactants are involved. In this case, we have 0.25 moles.
Step 3: Use the formula to calculate the heat absorbed: Heat absorbed = ΔH * n, where n is the number of moles.
Step 4: Substitute the values into the formula: Heat absorbed = -120 kJ * 0.25.
Step 5: Perform the multiplication: -120 kJ * 0.25 = -30 kJ.
Step 6: Interpret the result: Since the value is negative, it indicates that 30 kJ of heat is released, not absorbed.

Enthalpy Change (ΔH) – The heat change associated with a chemical reaction at constant pressure, where a negative ΔH indicates an exothermic reaction.
Mole Concept – Understanding how to relate the amount of substance (in moles) to the heat change in a reaction.
Heat Absorption vs. Release – Recognizing that a negative ΔH indicates heat is released, not absorbed.