You wish to monitor the progress of a reaction using pressures.Suppose 17.06 g N₂ (28.02 g/mol)and 1.228 g H₂ (2.016 g/mol)are initially present in a 20.0 L reaction vessel at 127 $\circ$ 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)$\to$ 2 NH₃(g)

Question

Quizplus · Accepted Answer

To find the percentage of N2 that has reacted, first calculate the initial moles of N2 and H2. Then, use the ideal gas law to find the initial total pressure. With the given total pressure at a certain point, determine the change in moles due to the reaction. Calculate the moles of N2 that have reacted and find the percentage of the initial moles.

You Wish to Monitor the Progress of a Reaction Using ∘\circ∘

You Wish to Monitor the Progress of a Reaction Using $\circ$