4.4 g of CO2 contains how many liters of CO2 at STP ?
a) 2.4 litre b) 2.24 litre
c) 44 Litre d) 22.4 litre
T=0⁰C = 273 K,
p= 1.01325•10⁵ Pa,
M=(12+16+16) •10³ = 40•10³ kg/mol.
V=mRT/Mp=
= 0.004•8.31•273/44•10⁻³•1.01325•10⁵=
=0.00204 m³= 2.04 L
2.4
To calculate the volume of CO2 at STP (Standard Temperature and Pressure) based on the given mass, you need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in this case, at STP it is 1 atm)
V = volume (what we are trying to find)
n = number of moles of the gas (to calculate n, we need to know the molar mass of CO2)
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (at STP it is 273 K)
First, let's find the number of moles of CO2.
To find the number of moles, divide the mass of CO2 by its molar mass.
The molar mass of CO2 is: 12.01 g/mol (carbon) + 2 * 16.00 g/mol (oxygen) = 44.01 g/mol
Number of moles = mass / molar mass
= 4.4 g / 44.01 g/mol
= 0.1 mol
Now, use the ideal gas law equation to find the volume (V):
V = nRT / P
V = (0.1 mol) * (0.0821 L·atm/(mol·K)) * (273 K) / (1 atm)
V = 2.2443 L
Therefore, the answer is approximately 2.24 liters.
So, the correct option is (b) 2.24 liters.