What kind of pressure would be exerted by 5 moles of water vapor if it were contained in a 0.5 liter bottle heated to 1000K?
To determine the pressure exerted by the water vapor, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = gas constant
T = temperature
First, let's gather the necessary information:
- Number of moles (n) = 5 moles
- Volume (V) = 0.5 liters
- Temperature (T) = 1000K
Next, we need to find the gas constant (R). The gas constant is commonly denoted by R and has a value of 0.0821 L·atm/(mol·K). However, you've provided the temperature in Kelvin, so we can use R = 8.314 J/(mol·K).
Plugging in the values into the equation:
PV = nRT
P * 0.5 = 5 * 8.314 * 1000
P * 0.5 = 41570
P = 41570 / 0.5
P ≈ 83,140 atm
Therefore, the pressure exerted by 5 moles of water vapor in a 0.5 liter bottle heated to 1000K would be approximately 83,140 atmospheres.