The heat of vaporization for benzaldehyde is 48.8 kj/mol, and its normal boiling point is 451.0 k. use this information to deter mine benzaldehyde's vapor pressure (in torr) at 61.5°c. report your answer to three significant digits.
1 answer:
Answer:
The vapor pressure of benzaldehyde at 61.5 °C is 70691.73 torr.
Explanation:
To solve this problem, we use Clausius Clapeyron equation: ln(P₁/P₂) = (ΔHvap / R) (1/T₁ - 1/T₂). The first case: P₁ = 1 atm = 760 torr and T₁ = 451.0 K. The second case: P₂ = <em>??? needed to be calculated </em> and T₂ = 61.5 °C = 334.5 K.ΔHvap = 48.8 KJ/mole = 48.8 x 10³ J/mole and R = 8.314 J/mole.K. Now, ln(P₁/P₂) = (ΔHvap / R) (1/T₁ - 1/T₂) ln(760 torr /P₂) = (48.8 x 10³ J/mole / 8.314 J/mole.K) (1/451 K - 1/334.5 K)
ln(760 torr /P₂) = (5869.62) (-7.722 x 10⁻⁴) = -4.53. (760 torr /P₂) = 0.01075 Then, P₂ = (760 torr) / (0.01075) = 70691.73 torr . So, The vapor pressure of benzaldehyde at 61.5 °C is 70691.73 torr.
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Explanation:
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1 atm = 760 mmHg
x atm = 30 mmHg
Upon solving for x;
x * 760 = 30 * 1
x = 30 / 760 = 0.03947 atm
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