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Answer:
Explanation:
Hi there,
To get started, let's first observe our rate law:
[tex]R=k[A]^2[B]^2[/tex] we typically use square brackets [x] for chemistry kinetics, because they specifically tell us we are dealing with concentrations.
This rate law is in fourth-order, because the concentrations powers add up to 4. We are not told the unit of time for this prompt (unless you know it), so I just assumed the time unit to be "time."
To calculate the reaction rate, we simply plug in the concentration of A and B into the rate law. k is the rate constant and stays the same for an individual reaction.
[tex]R=(0.1 \ M^{-3}*time^{-1})[1 \ M]^2[2 \ M]^2=0.4 \ M/time[/tex]
Thus, the rate of reaction with those concentrations is 0.4 M/time.
Notice, the rate constant does in fact have units of it own. The unit for k can be calculated by knowing that:
- Rate (R) must end up with units of concentration (M) per time.
- The concentrations raised to a power can be used to help solve for the units of k.
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The rate of reaction with those concentrations is 0.4 M/time.
What is the rate of a reaction?
The reaction rate is said to be the decrease in the concentration of the reactant or the increase in the concentration of the product per unit of time. Reaction rate measures how fast the reactant is used up or how fast the product is formed.
For a given reaction like
[tex]Mg(s) + O_2(g)[/tex] → [tex]2MgO(aq)[/tex]
The reaction rate is derived by measuring how fast the concentration of Mg and [tex]O_2[/tex] decreases or how fast the concentration of MgO increases. Mathematically reaction rate can be expressed as
Reaction rate = Δconcentration/ ΔTime
Rate=[tex]k(a)^2(b)^2[/tex] We typically use square brackets [x] for chemistry kinetics, because they specifically tell us we are dealing with concentrations.
This rate law is in fourth-order because the concentration powers add up to 4. We are not told the unit of time for this prompt (unless you know it), so I just assumed the time unit to be "time."
To calculate the reaction rate, we simply plug the concentration of A and B into the rate law. k is the rate constant and stays the same for an individual reaction.
Thus, the rate of reaction with those concentrations is 0.4 M/time.
Learn more about the rate of reaction here:
https://brainly.com/question/15766136
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