Which of the following is NOT an acceptable unit for reporting gas pressure?
1 answer:
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Answer:
The vapor pressure at temperature 363 K is 0.6970 atm
The vapor pressure at 383 K is 1.410 atm
Explanation:
To calculate of the reaction, we use clausius claypron equation, which is:
where,
= vapor pressure at temperature
= vapor pressure at temperature
= Enthalpy of vaporization
R = Gas constant = 8.314 J/mol K
1)
= initial temperature =363 K
= final temperature =373 K
Putting values in above equation, we get:
The vapor pressure at temperature 363 K is 0.6970 atm
2)
= initial temperature =373 K
= final temperature =383 K
Putting values in above equation, we get:
The vapor pressure at 383 K is 1.410 atm
Answer:
When the pressure increases to 90.0 atm , the volume of the sample is 0.01467L
Explanation:
To answer the question, we note that
P₁ = 1.00 atm
V₁ = 1.32 L
P₂ = 90 atm.
According to Boyle's law, at constant temperature, the volume of gas is inversely proportional to its pressure
That is P₁V₁ = P₂V₂
Solving the above equation for V₂ we have
that is V₂ =
=
or 0.01467L