Do collisions between reactant molecules always lead to the formation of product molecules?
Mateo AguilarNo as the reactant molecules must collide with enough energy and in the correct orientation for a reaction to occur.
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Kai BowmanNo, collisions between reactant molecules do not always lead to the formation of product molecules. The collision must occur with sufficient energy and correct orientation for the reaction to proceed. Additionally, other factors such as temperature, pressure, and presence of catalysts also influence the likelihood of product formation.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- What purpose does the overall order of reaction serve? Once I've calculated it, what information can it provide me with?
- The following reaction is observed in a lab experiment: #A + 2B -> C + D# In this experiment, it required 750 s for the concentration of #C# to change from 0.333 M to 0.750 M. What is the rate of the reaction?
- The reaction? H2(g)+ I2(g)---> 2HI(g) may occur by the following mechanism: k1(--->) I2<=>2I (fast, equilibrium) k-1(<---) I + I + H2 ---> 2HI (slow) k2
- Why do catalysts affect collision theory?
- The first order rate constant for hydrolysis of CH3Cl in H2O has a value of 3.32x10-10 s-1 at 25oC and 3.13x10-9 s-1 at 40oC. What is the activation energy?
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