Based on the data from the calorimetry experiment, the enthalpy change, ΔH of the reaction is -286 KJ .
The enthalpy change, ΔH of a reaction is the amount of heat evolved or absorbed when reactant molecules react to form products.
From the calorimetry experiment, the determined heat of combustion of 1.01 g of H2(g) reacting with excess O2(g), qsoln = 143 kJ.
Heat is evolved in the reaction, therefore the qsoln = -143 kJ
Equation of reaction is given as:
H2(g) + ½ O2(g) → H2O (l)
Molar mass of H = 1.01 g
Mass of H2 = 1.01 g × 2 = 2.02 g
ΔH of the reaction = -143 kJ × 2.02/1.01
ΔH of the reaction = -286 KJ
Therefore, the enthalpy change, ΔH of the reaction is -286 KJ .
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