Volume at N.T.P Of 0.22 gram of CO2 is same as that of.
A) 320MG of Gaseous SO2
B) 0.085g of NH3
C) 0.01g of H2
B) 0.085g of NH3
To compare the volumes of different gases at the same conditions, we can use the ideal gas law:
PV = nRT
Where:
P = pressure (constant for N.T.P)
V = volume
n = amount of substance in moles
R = ideal gas constant
T = temperature (constant for N.T.P)
Since the pressure and temperature are constant at N.T.P and we are comparing the same volume, we can simplify the equation to:
n₁/n₂ = M₁/M₂
Where:
n₁ = moles of CO₂
n₂ = moles of the gas we want to compare
M₁ = molar mass of CO₂
M₂ = molar mass of the gas we want to compare
First, we need to calculate the moles of CO₂.
Given:
Mass of CO₂ = 0.22 g
Molar mass of CO₂ = 44 g/mol
n₁ = (mass of CO₂) / (molar mass of CO₂)
= 0.22 g / 44 g/mol
= 0.005 mol
Now, let's compare the volumes of different gases:
A) For gaseous SO₂:
Given:
Mass of SO₂ = 320 mg
Molar mass of SO₂ = 64 g/mol
n₂ = (mass of SO₂) / (molar mass of SO₂)
= 320 mg / 1000 mg/g / 64 g/mol
= 0.005 mol
n₁ / n₂ = 0.005 mol / 0.005 mol
= 1
Since n₁ / n₂ = 1, the volume of 0.22 grams of CO₂ is the same as that of 320 mg of gaseous SO₂.
B) For NH₃:
Given:
Mass of NH₃ = 0.085 g
Molar mass of NH₃ = 17 g/mol
n₂ = (mass of NH₃) / (molar mass of NH₃)
= 0.085 g / 17 g/mol
= 0.005 mol
n₁ / n₂ = 0.005 mol / 0.005 mol
= 1
Since n₁ / n₂ = 1, the volume of 0.22 grams of CO₂ is the same as that of 0.085 grams of NH₃.
C) For H₂:
Given:
Mass of H₂ = 0.01 g
Molar mass of H₂ = 2 g/mol
n₂ = (mass of H₂) / (molar mass of H₂)
= 0.01 g / 2 g/mol
= 0.005 mol
n₁ / n₂ = 0.005 mol / 0.005 mol
= 1
Since n₁ / n₂ = 1, the volume of 0.22 grams of CO₂ is the same as that of 0.01 grams of H₂.
Therefore, the correct options are:
A) 320 mg of gaseous SO₂
B) 0.085 g of NH₃
C) 0.01 g of H₂