A 0.35 mol sample of an ideal gas is held in a vessel at 0.C and a pressure of 785 torr. What is the volume of the vessel? (R=62.36L x torr/mol x K)
PV=nRT
solve for V
785torr(V)= 0.35mol(62.36L)(273K)
answer: 7.6 L
is this correct?
i am not sure that the R(62.36L) is what is supposed to be there.
To find the volume of the vessel, we can use the Ideal Gas Law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in kelvin.
However, since the temperature is given in degrees Celsius, we need to convert it to kelvin. The conversion formula is T(K) = T(°C) + 273.15.
Given:
n = 0.35 mol
P = 785 torr
R = 62.36 L x torr/mol x K
T(°C) = 0°C
Converting temperature to kelvin:
T(K) = 0°C + 273.15 = 273.15 K
Now we can substitute the values into the Ideal Gas Law equation and solve for V:
PV = nRT
V = (nRT) / P
= (0.35 mol * 62.36 L x torr/mol x K * 273.15 K) / 785 torr
≈ 7.86 L
Therefore, the volume of the vessel is approximately 7.86 L.