When all are gaseous, one may use L as if L = moles, a good short cut to remember. Second, we must make sure both are at the same pressure; that can be accomplished by changing H2 to 1.00 atm. 1L H2 @ 2.00 atm = 2 L H2 @ 1.00 atm.
2NO(g) + 2H2(g) ® N2(g) + 2H2O(g)
Use the coefficients in the balanced equation to convert L NO and L H2 to L of either of the products.
2L NO x (1 mole N2/2 mols NO) = 2(1/2) = 1 mole N2 formed.
2L H2 X (1 mole N2/2 moles H2) = 2(1/2) = 1 mol N2 produced.
Therefore, neither is the limiting reagent. Or we could say both are limiting reagents.
2.00 L of NO(g) at 1.00 atm and 25°C is reacted with 1.00 L of H2(g) at 2.00 atm and 25°C according to the following unbalanced equation.
NO(g) + H2(g) ® N2(g) + H2O(g)
Which, if either, is the limiting reactant?
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