UNIT 3: Chemical Kinetics
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Reaction rate depends on:
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Rate constant increases with:
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Higher Ea means:
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Slope of Arrhenius plot is:
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Plot of ln k vs 1/T is:
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Catalyst decreases:
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Increase in temperature increases:
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Ea unit is:
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A is called:
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Arrhenius equation is:
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First-order reaction never:
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For zero order, rate decreases due to:
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Half-life formula for first order:
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Slope of first-order graph is:
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First-order reaction graph (ln[A] vs t) is:
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Graph of zero order is:
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Half-life for zero order depends on:
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Half-life for first order:
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First-order equation:
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Zero-order equation:
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Rate law for elementary reaction:
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Rate constant is independent of:
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Order of reaction for A → B is 1, half-life is:
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Rate constant depends on:
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Rate law cannot be predicted from:
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Order of complex reaction:
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Units of k depend on:
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Pseudo first-order reaction involves:
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If rate quadruples when concentration doubles → order:
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If rate doubles when concentration doubles → order is:
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Order of reaction can be negative in:
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Molecularity applies to:
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Rate = k → order is:
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Rate = k[A][B] → order is:
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Rate = k[A]² → order is:
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Rate law is:
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Collision theory explains:
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Activation energy is:
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Reaction rate doubles when temperature increases by ~:
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Unit of rate constant for first-order reaction:
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For zero-order reaction, rate is:
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Order is determined by:
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Order of reaction can be:
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Molecularity is always:
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Catalyst affects:
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Rate of reaction increases with increase in:
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Instantaneous rate is determined at:
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Average rate is measured over:
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Unit of rate of reaction is:
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The rate of a reaction is expressed as:
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