Pressure of pure A at 85 (degrees)C is 500 mmHg, what is the vapor pressure of pure B at this temperature?
A)336 mmHg
B)960 mmHg
C)576 mmHg
I apologize but the rest of the answer choices are:
D)260 mmHg
E)933 mmHg
Read your question and explain what it means. You give info for A and ask a question about B with no more info.My answer is to pick a number. It could be anything.
To find the vapor pressure of pure B at a given temperature, we can use the Clausius-Clapeyron equation. This equation relates the vapor pressures of two different substances at a given temperature.
The Clausius-Clapeyron equation is given by:
ln(P1/P2) = ΔHvap/R * (1/T2 - 1/T1)
Where:
P1 and P2 are the vapor pressures of the two substances.
ΔHvap is the molar enthalpy of vaporization.
R is the ideal gas constant (8.314 J/(mol*K)).
T1 and T2 are the temperatures at which the vapor pressures are measured in Kelvin.
In this problem, we are given the temperature (85 °C = 358 K) and the vapor pressure of pure A (500 mmHg). We need to find the vapor pressure of pure B.
First, we need to know the molar enthalpy of vaporization (ΔHvap) for substance B. This information is not given in the problem statement. Without the value of ΔHvap, we cannot calculate the vapor pressure of B using the Clausius-Clapeyron equation.
Therefore, the correct answer is not available in the given options.