Consider the reaction,

2AsH3(g) → 2As(g) + 3H2(g)

If the rate of formation of H2(g) is 0.090 mol·L—1·s—1, then the rate of formation of of As(g) is:

Question

Consider the reaction,

2AsH3(g)  →  2As(g) + 3H2(g)

If the rate of formation of H2(g) is 0.090 mol·L—1·s—1, then the rate of formation of of As(g) is:

BlackTom AI · Accepted Answer

The question presents the balanced chemical equation: 2AsH3(g) → 2As(g) + 3H2(g). To relate the rates, use the stoichiometric coefficients: for every 3 moles of H2 formed, 2 moles of As are formed.

Option 1: 0.030 mol·L—1·s—1. If you compare to the given rate of H2 formation (0.090), this option would imply a conversion factor of 0.030/0.090 = 1/3, which does not match the 3:2 ratio between H2 and As formation. Therefore this is inconsistent with the stoichiometry.

Option 2: 0.045 mol·L—1·s—1. This corresponds to a 0.045/0.090 = 1/2 ratio. The reaction shows a 3:2 ratio between H2 and As formation, not 1:2, so this option misuses the stoichiometric relationship.

Option 3: 0.060 mol·L—1·s—1. Here, 0.060/0.090 = 2/3. This exactly reflects the 2 moles of As formed per 3 moles of H2 produced in the balanced equation. The rate of formation of As(g) should be (2/3) times the rate of H2 formation, which computes to 0.060.

Option 4: 0.090 mol·L—1·s—1. This would imply the same rate as H2 formation, which would correspond to a 1:1 relationship. The stoichiometry does not support equal rates for H2 and As formation, since three hydrogens are produced for every two arsenic atoms formed.

Option 5: 0.135 mol·L—1·s—1. This would be more than the given H2 rate by a factor of 1.5, which again contradicts the 3:2 stoichiometric ratio and overshoots the expected rate based on the reaction coefficients.

In summary, the only option that aligns with the reaction’s 3 H2 produced for every 2 As formed is the one where the rate of As formation is (2/3) times the rate of H2 formation, yielding 0.060 mol·L—1·s—1.

Consider the reaction, 2AsH3(g) → 2As(g) + 3H2(g) If the rate of formation of H2(g) is 0.090 mol·L—1·s—1, then the rate of formation of of As(g) is:

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