Consider the reaction, 3H2 + N2 → 2NH3. If H2 is reacting at the rate of 0.15 M/s, at what rate is NH3 being produced?
0.15 x (2 molesNH3/3 moles H2) = 0.15 x (2/3)
To determine the rate at which NH3 is being produced, we need to analyze the stoichiometry of the reaction. The coefficients in the balanced equation provide the ratio of reactants and products. By examining these coefficients, we can determine how the reaction rates relate.
Given the balanced equation: 3H2 + N2 → 2NH3
The stoichiometric coefficients show that for every 3 moles of H2 reacting, 2 moles of NH3 are produced.
Now, let's relate the reaction rates using these stoichiometric coefficients.
The rate of the reaction can be expressed as the change in concentration with respect to time. Since the reaction involves gases, we use the term "pressure" in place of "concentration."
The given information states that the rate of H2 (reactant) is 0.15 M/s. However, we need the stoichiometric ratio between H2 and NH3 to determine the rate of NH3 production.
From the balanced equation, we can see that for every 3 moles of H2 reacting, 2 moles of NH3 are produced. Therefore, the stoichiometric ratio between the rate of H2 and NH3 is 3:2.
To find the rate at which NH3 is being produced, we multiply the rate of H2 by the stoichiometric ratio:
Rate of NH3 = (Rate of H2) x (2/3)
Rate of NH3 = 0.15 M/s x (2/3) = 0.10 M/s
Therefore, NH3 is being produced at a rate of 0.10 M/s.