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Calculate ΔSsurr when on mole of methanol (CH3OH) is formed from its elements under standard conditions if ΔfH0(CH3OH) = -238.9 J mol-1.

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Given : 

Number of moles of ethanol, 

(C2H5OH) = n = 1 mol 

ΔfH0(CH3OH) = -238.9 kJ mol-1

= -238.9 × 103J mol-1

Temperature = T = 298 K

ΔS = ?

ΔSsurr = ?

Since ΔfH0 is negative, 

The reaction for the formation of one mole of C2H5OH is exothermic. 

As heat is released to the surroundings,

ΔH0surr = + 238.9 kJ mol-1

∴ ΔSsurr\(\frac{ΔH^0_{surr}}{T}\) \(\frac{+238.9\times 10^3}{298}\)

= +801.7JK-1

Thus,

Entropy of the surroundings increases.

∴ ΔSsurr = +801.7JK-1

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