what is the volume of oxygen gas at STP from the decomposition of 1.70 g of sodium nitrate (85.00 g/mol)?
MOlar mass of NaNO3 = At.mass of Na + At.mass of N + (3xAt.mass of O )
= 23 + 14 + (3x16)
= 85 g/mol
Given mass of NaNO3 = 1.70 g
So number of moles of NaNO3 = mass/molar mass
= 1.70 g / 85 (g/mol)
= 0.02 mol
The decomposition of sodium nitrate is : 2 NaNO3 ----> 2NaNO2 + O2
According to the balanced equation ,
2 moles of NaNO3 produces 1 mole of oxygen
0.02 moles of NaNO3 produces M mole of oxygen
M = ( 0.02x1) / 2
= 0.01 moles of Oxygen
Calculation of number of moles of Oxygen :
We know that PV = nRT
Where
T = Temperature = 273 K
P = pressure = 1.0 atm
n = No . of moles = 0.01
R = gas constant = 0.0821 L atm / mol - K
V= Volume of the gas = ?
Plug the values we get V = (nRT) / P
= ( 0.01x0.0821x273) / 1.0
= 0.224 L
Therefore the volume of oxygen gas liberated is 0.224 L = 224 mL
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