Question

The vapor pressure of a given substance is doubled as the temperature changes from 27.5 to 62.3 degrees Celsius. Calculate the vapor formation enthalpy of the substance, assuming it is independent of temperature.

Answer #1

Choose the substance with the lowest vapor pressure at a given
temperature.
CO2
CaI2
BF3
Ar
PF5

The vapor pressure of a substance is measured over a range of
temperatures. A plot of the natural log of the vapor pressure
versus the inverse of the temperature (in Kelvin) produces a
straight line with a slope of −3.45×103 K . Find the enthalpy of
vaporization of the substance.

The vapor pressure of a liquid in a certain temperature range is
given by the formula ln(p)=a-b/T, where a and b are constant. Find
the enthalpy of vaporization of the liquid. (Hints:
Clausius-Clapeyron equation; p is the numerical value of the
pressure, i.e. it is dimensionless.)

The vapor pressure of a liquid doubles when the temperature is
raised from 91° C to 99° C. At what temperature will the vapor
pressure be four times the value at 91° C?. Answer should be in
Celsius.

The vapor pressure, p, of a compound varies with temperature as
follows
T / oC 0 20 40 50 70 80 90
100
p/ kPa 1.92 6.38 17.7 27.7 62.3
89.3 124.9 170.9
What are the (a) normal boiling
point and (b) the enthalpy of vaporization for this
compound.

The vapor pressure of a liquid in the temperature range 200K to
280K was found to fit the expression: ln(P) = 16.235-2601.8 / T
where P is in torr and T in kelvin. Calculate the enthalpy of
vaporization of the liquid and the normal boiling temperature.

A 1-m3 tank contains 1.042 kg of water vapor at pressure 200
kPa. Determine the temperature in degrees celsius (˚C) using the
van der Waals equation.

A.) The vapor pressure of a substance is 2.00x10^2 mmHg at 44.50
Celcius. What is its vapor pressure at 57 Celcius?
B.) At what temperature will the vapor pressure of the substance
be 5 times the pressure at 35.5 Celcius?
Hvap = 49.6 kJ/mol
I know the answer to letter A is 407, I am just unsure of how to
get the answer. Letter B I do not have an answer. Thank you in
advance.

Electrolysis problem. Calculate the partial pressure of H2
(using barometric pressure and vapor pressure of water) and the
Faradays required to generate 0.01358 moles of hydrogen gas given
the following information.
10 mL of 3 M H2SO4 was diluted in 100 ml. 49.8 mL of this
solution was used in electrolysis (initial buret reading was at 50
mL and final was at 0.2). The electrolysis was conducted at 20 V
for seven minutes and forty seconds. I calculated the moles...

At 50.14 K a substance has a vapor pressure of 258.9 torr.
Calculate its heat of vaporization in kJ/mol it if has a vapor
pressure of 161.2 torr at 277.5 K.

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