The gas-phase conversion of nitric oxide and hydrogen to nitrogen and water foll
ID: 963034 • Letter: T
Question
The gas-phase conversion of nitric oxide and hydrogen to nitrogen and water follows the reaction
k
NO(g) + H2(g) ½ N2(g) + H2O(g)
The rate of production of nitrogen as a function of initial reactant pressures is shown in the table at right. Is this reaction favorable under standard state conditions?
Select one:
Can't tell from the information given
It is favorable in the direction written
It is favorable in the opposite direction to the way it is written
The rate of production of nitrogen as a function of initial reactant pressures is shown in the table at right. Is this reaction favorable under standard state conditions?
Run P0H2(kPa) P0 NO (kPa) Rate (kPa/s) 1 53.3 40.0 0.137 2 53.3 20.3 0.033 3 38.5 53.3 0.213 4 19.6 53.3 0.105Explanation / Answer
Let us consider run (1) and (2) where the pressure of Hydrogen is kept fixed.
When the pressure of Nitric Oxide is halved the reaction rate is reduced 4 times.
Therefore, the rate is second order with respect to NO.
Let us consider run (3) and (4) where the pressure of Nitric Oxide is kept fixed.
When the pressure of Hydrogen is halved the reaction rate is reduced to half also.
Therefore, the rate is first order with respect to H2.
Hence, the rate law is expressed as r = k [H2][NO]2.
As for both the reactants the reaction rate increases with increase in the pressure the reaction will go in the forward direction under standard condition.
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