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:
d. Because those chemicals are easily made when CO2 reacts with water, forming H2CO3 (via carbonic anhydrase
Answer:
<h2>Hi there !</h2>
<h2>C. HCl</h2>
Explanation:
<h2>Reason :-</h2>
<h2>Salts are strong electrolytes, so they undergo complete dissociation.</h2><h3>Hope it helps u.....</h3><h3>Stay safe, stay healthy and blessed</h3><h3>Have a good day</h3><h3>Thank you ~</h3>
Answer:
Explanation:
Hello there!
In this case, since the titration of acids like KHP with bases like NaOH are performed in a 1:1 mole ratio, it is possible for us to know that their moles are the same at the equivalence point, and the concentration, volume and moles are related as follows:
Thus, by solving for the volume of the base as NaOH, we obtain:
Best regards!
Answer:
False
Explanation:
My opinion is False and im not sure
