If the enthalpy change (ΔH) for a reaction is -150 kJ and the reaction occurs at

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What’s inside this PDF?

Question: If the enthalpy change (ΔH) for a reaction is -150 kJ and the reaction occurs at constant pressure, how much heat is released when 3 moles of reactants are consumed?

Options:

50 kJ
150 kJ
450 kJ
300 kJ

Correct Answer: 450 kJ

Solution:

Heat released = ΔH * n = -150 kJ * 3 mol = -450 kJ.

If the enthalpy change (ΔH) for a reaction is -150 kJ and the reaction occurs at

Practice Questions

If the enthalpy change (ΔH) for a reaction is -150 kJ and the reaction occurs at constant pressure, how much heat is released when 3 moles of reactants are consumed?

50 kJ
150 kJ
450 kJ
300 kJ

Questions & Step-by-Step Solutions

If the enthalpy change (ΔH) for a reaction is -150 kJ and the reaction occurs at constant pressure, how much heat is released when 3 moles of reactants are consumed?

Step 1: Understand that ΔH (enthalpy change) tells us how much heat is released or absorbed during a reaction.
Step 2: Note that a negative ΔH value means heat is released. In this case, ΔH = -150 kJ.
Step 3: Identify how many moles of reactants are involved. Here, we have 3 moles.
Step 4: Use the formula to calculate the total heat released: Heat released = ΔH * number of moles.
Step 5: Plug in the values: Heat released = -150 kJ * 3 moles.
Step 6: Calculate the result: Heat released = -450 kJ.

Enthalpy Change – Understanding that ΔH represents the heat absorbed or released during a reaction at constant pressure.
Stoichiometry – Applying stoichiometric principles to calculate heat based on the number of moles of reactants.

If the enthalpy change (ΔH) for a reaction is -150 kJ and the reaction occurs at

What’s inside this PDF?

If the enthalpy change (ΔH) for a reaction is -150 kJ and the reaction occurs at

Practice Questions

Questions & Step-by-Step Solutions

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