The following reaction is investigated (assume an ideal gas mixture) . 2N₂O(g) + N₂H₄(g) 3N₂(g) + 2H₂O(g)
Initially there are 0.08 mol of N₂O and 0.29 mol of N₂H₄, in a 20.0-L container. If there is 0.050 mol of N₂O at equilibrium, how many moles of N₂ are present at equilibrium?

Question

The following reaction is investigated (assume an ideal gas mixture) . 2N₂O(g) + N₂H₄(g)

The following reaction is investigated (assume an ideal gas mixture) . 2N<sub>2</sub>O(g) + N<sub>2</sub>H<sub>4</sub>(g) 3N<sub>2</sub>(g) + 2H<sub>2</sub>O(g) Initially there are 0.08 mol of N<sub>2</sub>O and 0.29 mol of N<sub>2</sub>H<sub>4</sub>, in a 20.0-L container. If there is 0.050 mol of N<sub>2</sub>O at equilibrium, how many moles of N<sub>2</sub> are present at equilibrium? A) 0.053 B) 0.045 C) 0.12 D) 0.030 E) 0.15

3N₂(g) + 2H₂O(g)
Initially there are 0.08 mol of N₂O and 0.29 mol of N₂H₄, in a 20.0-L container. If there is 0.050 mol of N₂O at equilibrium, how many moles of N₂ are present at equilibrium?

Quizplus · Accepted Answer

The Answer of The following reaction is investigated (assume an ideal gas mixture). 2N₂O(g) + N₂H₄(g) 3N₂(g) + 2H₂O(g) Initially there are 0.08 mol of N₂O and 0.29 mol of N₂H₄, in a 20.0-L container. If there is 0.050 mol of N₂O at equilibrium, how many moles of N₂ are present at equilibrium?

The Following Reaction Is Investigated (Assume an Ideal Gas Mixture)