Solve PV=nRT for V on Venus at STP

[amiv4]

Homework Statement

The conditions of standard temperature and pressure STP are a temperature of 0.00 C and a pressure of 1.00 atm.

For a scientist on Venus, an absolute pressure of 1 Venusian-atmosphere is 92 Earth-atmospheres. Of course she would use the Venusian-atmosphere to define STP. Assuming she kept the same temperature, how many liters would 1 mole of ideal gas occupy on Venus?

The Attempt at a Solution

PV=nRT
(1/92 atm)V=1 mol(.08205746 (L atm)/(K mol))(273.15 C)
V=2062.086

but that isn't right

 

[D H]

The pressure at the surface of Venus is 92 atmospheres, not 1/92^nd of an atmosphere.

 

[tomcue]

because it doesn't take into account the different temperature and pressure on Venus.

To solve PV=nRT for V on Venus at STP, we need to consider the different temperature and pressure conditions on Venus compared to Earth. The temperature on Venus is much higher than 0.00 C, so we need to use the corresponding temperature in Kelvin. Additionally, the pressure on Venus is not 1.00 atm, but rather 92 times that of Earth's atmosphere. Therefore, the correct equation to use is:

(1/92 atm)V = 1 mol (0.08205746 (L atm)/(K mol))(737.15 K)

Solving for V, we get:

V = 15.81 liters

So, 1 mole of an ideal gas on Venus at STP would occupy 15.81 liters, which is significantly larger than the volume on Earth due to the higher temperature and pressure. It is important to consider the specific conditions of a planet when solving equations like PV=nRT.