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Calculate the heat involved with 96 g HBr (mw = 80.9 g/mol) in the following reaction:rn2kbr + H2SO4 + 120 kj → K2SO4 + 2hbr.
Accepted Answer
The reaction given is:
2KBr + H2SO4 + 120 kJ → K2SO4 + 2HBr
This equation indicates that the reaction is endothermic, meaning it absorbs heat from the surroundings. The 120 kJ value represents the enthalpy change (ΔH) for the reaction, which is positive for endothermic processes. This means that 120 kJ of heat is absorbed for every 2 moles of HBr produced.
To calculate the heat involved with 96 g of HBr, we need to follow these steps:
1. Convert grams of HBr to moles:
Moles of HBr = (mass of HBr) / (molar mass of HBr) = 96 g / 80.9 g/mol = 1.18 mol
2. Determine the heat absorbed for the given amount of HBr:
Since the reaction releases 120 kJ for 2 moles of HBr, the heat absorbed for 1.18 moles of HBr is:
Heat absorbed = (1.18 mol HBr)
(120 kJ / 2 mol HBr) = 70.8 kJ
Therefore, the heat involved in the reaction with 96 g of HBr is 70.8 kJ.
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