Question

A chemist measures the energy change ΔH during the following reaction: C₃H₈(g)+502(g) → 3 CO₂(g) + 4H₂O(1) Use the information to answer the following question. Suppose 24.5 g of C₃H₈ react. Calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. kJ ΔΗ= -2220. kJ x10 X S

Answer 1

To find the heat released for 24.5 g of C3H8, convert the mass to moles and multiply by the ΔH per mole. The heat released is approximately 1233.1 kJ.

Step-by-step explanation:

To calculate the amount of heat released when 24.5 g of C3H8 reacts, we must relate the given mass to moles using the molar mass of C3H8 (propane). The molar mass of propane is 44.09 g/mol. By dividing the mass of propane by its molar mass, we find the number of moles that will react:

1. Calculate moles of C3H8: Moles = Mass / Molar Mass = 24.5 g / 44.09 g/mol
2. Determine the moles of C3H8: Moles = 0.555 mol
3. Apply the enthalpy change (ΔH) per mole for the reaction: For the combustion of 1 mole of propane, ΔH = -2220 kJ. Thus, the heat released for 0.555 moles is: Heat released = -2220 kJ/mol * 0.555 mol
4. Calculate the total heat released: Heat released ≈ -1233.1 kJ

Therefore, when 24.5 g of C3H8 reacts, approximately 1233.1 kJ of heat will be released.