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.
Answer:
20
Explanation:
Atoms have the same amount of electrons as they have protons. Therefore, if an atoms has 20 protons, it should have 20 electrons.
Answer:
2, stronger hydrogen bonding
Explanation:
Energy is little Electric molecules in the air when a negative charge and a positive charge touch that makes
Energy
Answer:
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Explanation:
<u>1) Chemical equilibrium</u>
- 2Hg (l) + O₂ (g) ⇄ 2HgO (s) (the double arrow indicates an equilibrium reaction)
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<u>2) Equilibrium constant, Kc:</u>
- The equilibrium constant, Kc, is equal to product of the concentrations of each product,each raised to its stoichiometric coefficient / product of the concentrations of each reactant each raised to its stoichiometric coefficient.
- Since the concentrations of liquid and solid substances remain practically constant, their value is incorporated into the constant Kc, and the equation only uses the concentrations of the aqueous or gaseous substances.
Thus, the equation to use is:
<u>3) Determine the concentration of O₂ (g)</u>
- M = number of moles / volume in liters
- Number of moles = mass in grams / molar mass
- Number of moles of O₂ (g) = 13.4 g / 32.00 g/mol = 0.419 mol
- M = 0.419 mol / 5.2 liter = 0.0806 mol / liter = 0.0806 M
<u>4) Compute Kc</u>
- Kc = 1 / 0.0 806 M = 12.4 M⁻¹ ← answer
