Find the volume 2.2g CO2 occupues at stp
To find the volume of 2.2g of CO2 at STP (Standard Temperature and Pressure), we need to use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (at STP, it is 1 atm)
V = Volume (what we are trying to find)
n = Number of moles of the gas
R = Ideal gas constant (0.0821 L·atm/(mol·K))
T = Temperature (at STP, it is 273K)
First, we need to calculate the number of moles of CO2:
n = mass / molar mass
The molar mass of CO2 is:
C = 12.01 g/mol
O = 16.00 g/mol
Molar mass of CO2 = 12.01 g/mol + (16.00 g/mol * 2) = 44.01 g/mol
n = 2.2 g / 44.01 g/mol = 0.05 mol
Now we can plug the values into the ideal gas law equation:
(1 atm) * (V) = (0.05 mol) * (0.0821 L·atm/(mol·K)) * (273K)
V = (0.05 mol) * (0.0821 L·atm/(mol·K)) * (273K) / (1 atm)
V ≈ 1.186 L
Therefore, 2.2g of CO2 occupies approximately 1.186 L at STP.
To find the volume of 2.2 grams of CO2 at STP (Standard Temperature and Pressure), we need to use the ideal gas law.
The ideal gas law is given by the equation:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature in Kelvin
At STP, the temperature is 273.15 Kelvin and the pressure is 1 atmosphere.
To solve for the volume, we need to find the number of moles of CO2. To do this, we can use the molar mass of carbon dioxide.
The molar mass of CO2 is calculated by adding the atomic masses of carbon (12.01 g/mol) and oxygen (16.00 g/mol) together.
Molar mass of CO2 = 12.01 g/mol + 16.00 g/mol + 16.00 g/mol = 44.01 g/mol
Now we can calculate the number of moles of CO2:
Number of moles = mass / molar mass
Number of moles = 2.2 g / 44.01 g/mol ≈ 0.05 mol
Now we can substitute the values into the ideal gas law equation:
PV = nRT
(1 atm) * V = (0.05 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K)
V ≈ 1.18 L
Therefore, the volume of 2.2 grams of CO2 at STP is approximately 1.18 liters.