This rate law suggests its rate to be direct proportional to H2 concentration, thus halving this would implicate a halved reaction rate.
The rate would be one-fourth. Apex
The rate would also behalved
The rate would be four times larger. Impossible.
The reaction rate would decrease
If you held your breath, the concentration of oxygen in your lungs would decrease. The concentration of carbon dioxide would increase in your lungs.
None. A catalyst affects only the rate of reaction, and if the reaction is already at equilibrium, the net rate of the reaction is zero and remains so after a catalyst is added.
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
The one with the larger mass would pull the halved mass one toward it