A gas has a volume of 91 ml at a temperature of 91°C. This gas is kept at constant pressure but its temperature is reduced to 0.0°C. At this temperature the volume of the gas will be approximately
Charles Law?
V1/V2=T1/T2
work it in Kelvins, not Celcius.
(P1V1)/T1 = (P2V2)/T2
Since pressure is constant, just ignore it (either omit it from the formula OR put a 1 for both P1 and P2). Don't forget to use Kelvin for T.
To find the approximate volume of the gas at 0.0°C, we can use the combined gas law equation, which relates the initial and final conditions of a gas when pressure and amount of gas are kept constant. The equation is as follows:
(P₁ * V₁) / T₁ = (P₂ * V₂) / T₂
Where:
P₁ and P₂ are the initial and final pressures of the gas, which are kept constant.
V₁ and V₂ are the initial and final volumes of the gas, respectively.
T₁ and T₂ are the initial and final temperatures of the gas, respectively.
Given:
V₁ = 91 ml
T₁ = 91°C = 91 + 273.15 = 364.15 K (converting to Kelvin)
T₂ = 0.0°C = 0.0 + 273.15 = 273.15 K (converting to Kelvin)
Since the pressure is constant, we can rewrite the equation as:
V₁ / T₁ = V₂ / T₂
Substituting the given values:
91 ml / 364.15 K = V₂ / 273.15 K
To solve for V₂, we can cross multiply and simplify:
91 ml * 273.15 K = V₂ * 364.15 K
V₂ = (91 ml * 273.15 K) / 364.15 K
Calculating this expression:
V₂ ≈ 68.368 ml
Therefore, at a temperature of 0.0°C, the volume of the gas will be approximately 68.368 ml.