Answer:
The value of the partial pressure of the oxygen = 690 torr
Explanation:
Total pressure of the mixture of gases = 736 torr
The partial pressure of water vapor = 46 torr
From the law of pressure we know that
Total pressure = The partial pressure of water vapor + The partial pressure of oxygen
Put the values of pressures in above equation we get,
⇒ 736 = 46 +
⇒ = 736 - 46
⇒ = 690 torr
This is the value of the partial pressure of the oxygen.
Answer:
3.72L
Explanation:
Given parameters:
Initial volume V₁ = 3.9L
Condition = STP
Final temperature T₂ = -550°C
Final pressure P₂ = 880mmHg
Unknown:
Final volume V₂ = ?
Solution.
At standard temperature and pressure(STP), the:
Pressure = 1atm = 760mmHg
Temperature = 273K
Therefore, P₁ = 760mmHg
T₁ = 273K
The general gas law, is best to solve this problem. It is mathematically given as:
Let us take the units to the appropriate one;
-550°C = 273 + (-550) = -277K
Input the variables;
V₂ = 3.72L