In the reaction
2N2O5 → 4NO2 + O2
given that the rate law is v = k[N 2O5]
where v is the reaction rate or reaction velocity, calculate the rate of formation of NO 2 if the instantaneous rate of reaction is 1.7 x 10-6 mol L-1 s-1.
Subjects
Sections | |||
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Rate of Reaction | 11 mins | 0 completed | Learn Summary |
Average Rate of Reaction | 18 mins | 0 completed | Learn |
Arrhenius Equation | 16 mins | 0 completed | Learn Summary |
Rate Law | 38 mins | 0 completed | Learn Summary |
Integrated Rate Law | 52 mins | 0 completed | Learn Summary |
Collision Theory | 9 mins | 0 completed | Learn |
Additional Practice |
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Instantaneous Rate of Change |
Energy Diagram |
Catalyst |
Michaelis-Menten Equation |
Reaction Mechanism |
Identifying Reaction Order |
In the reaction
2N2O5 → 4NO2 + O2
given that the rate law is v = k[N 2O5]
where v is the reaction rate or reaction velocity, calculate the rate of formation of NO 2 if the instantaneous rate of reaction is 1.7 x 10-6 mol L-1 s-1.
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