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barxatty [35]
2 years ago
7

For a given reaction, ΔH=78.7kJ/mol, and the reaction is spontaneous at temperatures above the crossover temperature, 461K. The

value of ΔS= _______ J/mol⋅K, assuming that ΔH and ΔS do not vary with temperature.
Chemistry
1 answer:
TiliK225 [7]2 years ago
7 0

Answer:

171 J/mol.K

Explanation:

The spontaneity of a reaction depends on the Gibbs free energy (ΔG). If ΔG < 0, the reaction is spontaneous. The Gibbs free energy is related to the enthalpy (ΔH) and the entropy (ΔS) of the reaction through the following expression:

ΔG = ΔH - T.ΔS

where,

T is the absolute temperature

If ΔG < 0,

ΔH - T.ΔS < 0

ΔH < T.ΔS

ΔS > ΔH/T = (78.7 × 10³ J/mol)/461 K = 171 J/mol.K

ΔS must be at least 171 J/mol.K for the reaction to be spontaneous above 461 K.

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When a candle burns it produced 41,300 Joules per 1 gram. Use dimensional analysis to convert this to Calories per pound.
insens350 [35]

Answer:

4477381.7 calories/pound

Explanation:

It is given that,

When a candle burns it produced 41,300 Joules per 1 gram.

We need to convert it into calories per pound.

We know that,

1 cal = 4.184 J

⇒ 1 J = (1/4.184) cal

1 pound = 453.592 grams

⇒1 g = (1/453.592) pounds

Now,

41300\ \text{Joules per gram}=\dfrac{41300\ \text{Joules}}{\text{gram}}\\\\=41300\times \dfrac{\dfrac{1}{4.184}\ \text{calories}}{\dfrac{1}{453.592}\ \text{gram}}\\\\=4477381.7\ \text{calories/pound}

Hence, 41,300 Joules/gram = 4477381.7 calories/pound.

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