Consider two gases, A and B, are in a container at room temperature. What effect will the following changes have on the rate of
2 answers:
Explanation:
As it is given that two gases A and B are mixed together and kept in a container with constant volume.
Also, kinetic energy of molecules is directly related to temperature as follows.
K.E =
As kinetic energy is directly proportional to temperature. So, when there will be decrease in temperature then kinetic energy of molecules will also decrease leading to less number of collisions between the molecules.
Hence, there will be decrease in rate of reaction.
Thus, we can conclude that when temperature is decreased at a constant volume then rate of reaction will also decrease.
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Answer:
- False.
- False.
- True.
- True.
Explanation:
Hello, for each statement we state:
- An exponent of "2" means that if we double the concentration of the reactant the rate doubles as well.
FALSE because considering a rate law like:
The exponent of "2" powers the concentration to the second power, not doubles the rate law, thus, if C is 3, for k=1, r will be -9. On the other hand if the rate is like:
The rate will be -3, that is why the rate is not doubled when the "2" in concentration is present.
- Exponents in rate laws are based on the coefficients from the balanced equation.
FALSE because for nonelemental chemical reactions, the exponents do not match with each species' stoichiometric coefficients in the rate law.
- The rate constant, k, takes into account the effect of activation energy and temperature on the reaction.
TRUE, since the Arrhenius equation allows us to prove the effect of the activation energy and the temperature:
- Differential rate laws allow us to compare concentration and time.
TRUE as they are given like:
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