You wish to monitor the progress of a reaction using pressures.Suppose 17.06 g of N₂ (28.02 g/mol) and 1.228 g of H₂ (2.016 g/mol) are initially present in a 20.0 L reaction vessel at 127 C.Nitrogen and hydrogen can react to form ammonia (17.04 g/mol) according to the reaction shown.At a given point, the total pressure (the sum of the pressures of N₂, H₂, and NH₃ present) is 1.48 atm.What percentage of the initial N₂ has reacted? N₂ (g) =3 H₂ (g) $\rightarrow$ 2 NH₃ (g)

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The Answer of You wish to monitor the progress of a reaction using pressures.Suppose 17.06 g of N₂ (28.02 g/mol) and 1.228 g of H₂ (2.016 g/mol) are initially present in a 20.0 L reaction vessel at 127 C.Nitrogen and hydrogen can react to form ammonia (17.04 g/mol) according to the reaction shown.At a given point, the total pressure (the sum of the pressures of N₂, H₂, and NH₃ present) is 1.48 atm.What percentage of the initial N₂ has reacted? N₂ (g) =3 H₂ (g) $\rightarrow$ 2 NH₃ (g)

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