Answer:
16.48 mL.
Explanation:
From the question given above, the following data were obtained:
Initial pressure (P₁) = 1 atm
Initial temperature (T₁) = 0 °C
Initial volume (V₁) = 30 mL
Final temperature (T₂) = 27 ° C
Final pressure (P₂) = 2 atm
Final volume (V₂) =?
Next, we shall convert celsius temperature to Kelvin temperature. This can be obtained as follow:
T(K) = T(°C) + 273
Initial temperature (T₁) = 0 °C
Initial temperature (T₁) = 0 °C + 273
Initial temperature (T₁) = 273 K
Final temperature (T₂) = 27 °C
Final temperature (T₂) = 27 °C + 273
Final temperature (T₂) = 300 K
Finally, we shall determine the final volume of the gas. This can be obtained as:
Initial pressure (P₁) = 1 atm
Initial temperature (T₁) = 273 K
Initial volume (V₁) = 30 mL
Final temperature (T₂) = 300 K
Final pressure (P₂) = 2 atm
Final volume (V₂) =?
P₁V₁ / T₁ = P₂V₂ / T₂
1 × 30 / 273 = 2 × V₂ / 300
30 / 273 = 2 × V₂ / 300
Cross multiply
273 × 2 × V₂ = 30 × 300
546 × V₂ = 9000
Divide both side by 546
V₂ = 9000 / 546
V₂ = 16.48 mL
Therefore, the final volume of the gas is 16.48 mL.
