0.4 (mol/L)/s
A trapezoid has no intrinsic value.
It is 1/16.
1200SQM
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1 radian = 360/tau (or 180/pi) degrees.
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.
In a zero order overall process, the rate and rate constant will be the same. (Reaction order is an exponent, and if that exponent is "0" then the value is "1" and will cancel out.)
No, 0.01 is not written as 0.01% in percent rate. 0.01 in percent rate is 1%.
Chain Reaction - 1980 1980-04-01 was released on: USA: 1 April 1980
Chain Reaction - 1980 1980-05-01 was released on: USA: 1 May 1980
A + B --> C has non-elementary reaction rate equation -rA = kCACB1/2 The exponent of CA is 1, the exponent of CB is 1/2, for an overall reaction order of 1 + (1/2) = 1.5. Do not let the stoichiometric coefficients from the reaction mislead you. It has to do with the rate equation for a given reaction, not the (net) chemical reaction itself.
1. The rate of forward reaction = to the rate of backward reaction. 2. Concentration of the substance are constant.
The overall reaction order for k[A]^2[B][C] would be 4 Because [A] has a rate order of 2 [B] has a rate order of 1 [C] has a rate order of 1 And when you add them together... 2 + 1 + 1 You obtain four
temperature is proportional to 1/time taken for reaction to complete (rate of reaction)
the answer is rate
equilibrium means the rate of forward reaction = rate of backward reaction... there are three types of equilibrium 1. amount of products > amount of reactants 2. amount of products = amount of reactants 3. amount of products < amount of reactants
What indeed. Your "increased" rate has a lower value than your initial rate.