how to find the rate of any reaction?
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EXAMPLE 1
For the oxidation of ammonia
4NH3+3O2→2N2+6H2O
4NH33O22N26H2O
it was found that the rate of formation of N2 was 0.27 mol L–1 s–1.
At what rate was water being formed?
At what rate was ammonia being consumed?
SOLUTION
a) From the equation stoichiometry, Δ[H2O] = 6/2 Δ[N2], so the rate of formation of H2O is
3 × (0.27 mol L–1 s–1) = 0.81 mol L–1 s–1.
b) 4 moles of NH3 are consumed for every 2 moles of N2 formed, so the rate of disappearance of ammonia is
2 × (0.27 mol L–1 s–1) = 0.54 mol L–1 s–1.
Comment: Because of the way this question is formulated, it would be acceptable to express this last value as a negative number.
For the oxidation of ammonia
4NH3+3O2→2N2+6H2O
4NH33O22N26H2O
it was found that the rate of formation of N2 was 0.27 mol L–1 s–1.
At what rate was water being formed?
At what rate was ammonia being consumed?
SOLUTION
a) From the equation stoichiometry, Δ[H2O] = 6/2 Δ[N2], so the rate of formation of H2O is
3 × (0.27 mol L–1 s–1) = 0.81 mol L–1 s–1.
b) 4 moles of NH3 are consumed for every 2 moles of N2 formed, so the rate of disappearance of ammonia is
2 × (0.27 mol L–1 s–1) = 0.54 mol L–1 s–1.
Comment: Because of the way this question is formulated, it would be acceptable to express this last value as a negative number.
Answered by
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The initial rate of a reaction is the instantaneous rate at the start of thereaction (i.e., when t = 0). The initialrate is equal to the negative of the slope of the curve of reactant concentration versus time at t = 0.
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