The total energy of a system remains constant.
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.
I would like to help you, but you are not showing the options. just their letter.
Answer:
The calculations are in the explanation below.
The <em>steps </em>are:
- 1. Using a graduated pipette, accurately take 25mL of the 12.0M stock solution.
- 2. Pour the 25mL of stock solution into a 100 mL volumetric flask
- 3. Add distilled water up to the mark
- 4. Cap the flask with the stopper
- 5. Stirr by gently rotating the flask.
Explanation:
To make 100 mililiter of the 3.0M solution of sulfuric acid, first you must calculate the volume of the 12.0M stock solution that contains the same number of moles as the diluted solution.
For that, you use the dilution formula:
- number of moles = C₁V₁ = C₂V2
- V₁ = 3.0M × 100mL/12.0M = 25mL
Then, the steps are:
1. Using a graduated pipette, accurately take 25mL of the 12.0M stock solution.
2. Pour the 25mL of stock solution into a 100 mL volumetric flask
3. Add distilled water up to the mark
4. Cap the flask with the stopper
5. Stirr by gently rotating the flask.
Answer:
An atom is a particle of matter that uniquely defines a chemical element . An atom consists of cental nucleus that is usually surrounded by one or more electrons. Each electrons is negatively charged.
Hope this helps you! bye