A mass of gas occupies 20cm at5c and 760mmhg pressure what is its volume at30c and800mmhg pressure .
change temps to Kelvins.
combined gas law:
p1V1T2=P2V2T1
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5.5
To solve this problem, we can use the combined gas law, which states that the ratio of initial pressure to final pressure is equal to the ratio of initial volume to final volume, multiplied by the ratio of final temperature to initial temperature.
The formula for the combined gas law is:
(P₁ * V₁) / (T₁) = (P₂ * V₂) / (T₂)
Where:
P₁ = initial pressure
V₁ = initial volume
T₁ = initial temperature
P₂ = final pressure
V₂ = final volume
T₂ = final temperature
Now, let's plug in the given values into the formula:
P₁ = 760 mmHg
V₁ = 20 cm³
T₁ = 5°C + 273.15 = 278.15 K
P₂ = 800 mmHg
T₂ = 30°C + 273.15 = 303.15 K
Plug in the values into the formula:
(760 mmHg * 20 cm³) / (278.15 K) = (800 mmHg * V₂) / (303.15 K)
Now, rearrange the formula to solve for V₂ (final volume):
V₂ = [(760 mmHg * 20 cm³ * 303.15 K) / (278.15 K * 800 mmHg)]
Now, solve the equation:
V₂ = (18,450 mmHg * cm³ * K) / (222,520 mmHg)
Calculating:
V₂ ≈ 0.0829 cm³
Therefore, the volume of the gas at 30°C and 800 mmHg pressure is approximately 0.0829 cm³.