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It will decrease by half.
The rate would be four times larger. Impossible.
Since the reaction is first order with respect to H2, if the concentration of H2 were halved, the rate of the reaction would be halved. This can be seen by entering one for each value in the rate equation, then changing the value of [H2] to 1/2 while keeping the other values the same: The rate changes from 1 to 1/2.
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The rate would quadruple (increase by a factor of 4). This is because the rate depends on the SQUARE of the concentration of NO.
This rate law suggests its rate to be direct proportional to H2 concentration, thus halving this would implicate a halved reaction rate.
It will decrease by half.
The rate would also behalved
The rate would be four times larger. Impossible.
The rate would be four times larger. Impossible.
The reaction rate would decrease
Since the reaction is first order with respect to H2, if the concentration of H2 were halved, the rate of the reaction would be halved. This can be seen by entering one for each value in the rate equation, then changing the value of [H2] to 1/2 while keeping the other values the same: The rate changes from 1 to 1/2.
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The wavelength would double.
circumference would be halved, area would be one fourth of original , andvolume would be one eighth of original.
The rate would quadruple (increase by a factor of 4). This is because the rate depends on the SQUARE of the concentration of NO.
The rate would be four times larger