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11.00g of Compound X with molecular formula C4H6 are burned in a constant-pressure calorimeter containing 35.00kg of water at 25°C. The temperature of the water is observed to rise by 3.396°C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25°C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits

Answer :

The standard heat (Δ[tex]H_{f}[/tex]) of compound formed will be 2441.34 KJ.

Given in question:

Molecular formula of [tex]C_{4}H_{4}[/tex] = 54 g/mole

mass of water = 35.00 kg,

Specific heat = 4.184 J/g °C,

Change in temperature = 3.396°C.

Heat energy is calculated using this formula: Q = msΔT.

=>35×1000 × 4.184 × 3.396 = 497.31 KJ.

∴ Standard heat of the compound X will be

=> Δ[tex]H_{f}[/tex] = (54 × 497.31)/11 = 2441.34 KJ.

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