Consider the following reaction: A + B → products. The rate law was found to be rate = k[A][B]^2. A)If the concentration of A is doubled while the concentration of B is kept constant, how will this affect the rate of the reaction? How will this affect the time required for the reaction to reach completion? B)If the concentration of B is doubled while the concentration of A is kept constant, how will this affect the rate of the reaction? How will this affect the time required for the reaction to reach completion? C)If the concentration of B is doubled while the concentration of A is halved, how will this affect the rate of the reaction? How will this affect the time required for the reaction to reach completion?
- Consider the following reaction: A + B → products. The rate law was found to be rate = k[A][B]^2.
A)If the concentration of A is doubled while the concentration of B is kept constant, how will this affect the
B)If the concentration of B is doubled while the concentration of A is kept constant, how will this affect the rate of the reaction? How will this affect the time required for the reaction to reach completion?
C)If the concentration of B is doubled while the concentration of A is halved, how will this affect the rate of the reaction? How will this affect the time required for the reaction to reach completion?
Rate of a chemical reaction is defined as the speed with which the reaction proceeds. It determines that a reaction is slow or fast.
Rate law of a reaction is directly proportional to the product of the concentration of the reactants raised to some power. The sum of the powers of the concentrations of the reactants give the order of the reaction. Order of the reaction can be determined experimentally.
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