how many moles are in 5L of CO2 at STP?
To determine the number of moles in 5L of CO2 at STP (Standard Temperature and Pressure), we will make use of the ideal gas law equation: PV = nRT, where P represents pressure, V represents volume, n represents moles, R represents the ideal gas constant, and T represents temperature.
At STP, the pressure is 1 atmosphere (atm), the temperature is 273.15K (0 degrees Celsius), and R is equal to 0.0821 L·atm/mol·K.
Given:
V = 5L
P = 1 atm
T = 273.15K
Using the ideal gas law equation: PV = nRT
Substituting the known values:
(1 atm) * (5L) = n * (0.0821 L·atm/mol·K) * (273.15K)
Simplifying the equation:
5 = 0.0821 * 273.15 * n
Dividing both sides of the equation by (0.0821 * 273.15):
5 / (0.0821 * 273.15) = n
Calculating the value on the left side of the equation:
n ≈ 0.224 moles
Therefore, there are approximately 0.224 moles in 5L of CO2 at STP.
To calculate the number of moles in 5L of CO2 at STP (Standard Temperature and Pressure), we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L atm / K mol)
T = temperature (in Kelvin)
At STP, the pressure is 1 atmosphere and the temperature is 273.15 K.
So we have:
1 atm * 5 L = n * 0.0821 L atm / K mol * 273.15 K
Simplifying the equation:
5 atm L = n * 22.414 L atm / K mol
Now, let's solve for n:
n = (5 atm L) / (22.414 L atm / K mol)
n = 0.223 moles
Therefore, there are approximately 0.223 moles of CO2 in 5L of gas at STP.