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The rate of a reaction can be expressed using the rate law equation, which typically takes the form ( \text{Rate} = k[A]^m[B]^n ), where ( k ) is the rate constant, and ( A ) and ( B ) are the concentrations of the reactants raised to their respective powers ( m ) and ( n ). In this case, if ( k = 3 ), ( [A] = 2 , \text{M} ), and ( [B] = 2 , \text{M} ), and assuming ( m ) and ( n ) are both 1 (first-order with respect to both reactants), the rate would be calculated as ( \text{Rate} = 3 \times (2)^1 \times (2)^1 = 3 \times 2 \times 2 = 12 , \text{M/s} ). If the orders of the reaction are different, the calculation would change accordingly.

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1d ago

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