i>clicker: Calculate the volume of N2 necessary to react with
9.0 L of H2 gas at 450 K and 5.00 atm.
a) 9.0 L
b) 3.0 L
c) 27.0 L
d) 1.0 L
N2 (g) + 3H2 (g) -----------> 2NH3 (g)
1 mole of nitrogen reacts with 3 moles of hydrogen gas
Given 9 litres of H2 gas.
Temperature = 450 K
Pressure = 5 atm
Applying ideal gas equation for H2
PV = nRT , here R is the gas constant = 0.0821 atm L / mol*K
=> 5*9 = n *0.0821*450
=> n = 1.22 moles of N2
So , 3 moles of H2 reacts with 1mole of N2
1.22 moles of H2 requires 1.22 /3 moles of N2 = 0.406 moles
Again applying ideal gas equation for N2 for the given conditions we get
PV = nRT
=> 5V = 0.406*0.0821*455
=> V = 3.03 litres = 3 litres approx. Ans
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