Answer:
Slow step is the rate determining step.
Explanation:
In general a reaction occurs in two or more elementary steps. Rate of reaction of each step is different. In chemical kinetics, rate of overall reaction is decided by rate of slowest step.
Consider the given reaction,
The given reaction has two elementary steps.
Step 1: H2(g)+ICl(g)→HI(g)+HCl(g) (slow)
Step 2: HI(g)+ICl(g)→I2(g)+HCl(g) (fast)
Step 2 is fast and completes in no time. Whereas step 1 is slow. As reaction cannot go to completion without step 1, so rate of the reaction is decided by rate of the slowest step.
Answer: An existing theory is modified so that it can explain both the old and new observations.
Explanation:
<u>Answer:</u> of the reaction will be negative, of the reaction will be positive and of the reaction will be negative.
<u>Explanation:</u>
Thermodynamic properties are enthalpy change , entropy change and Gibbs free energy
Exothermic reactions are defined as the reactions in which energy is released in the form of heat. The enthalpy change of the reaction comes out to be negative for this kind of reaction.
Entropy change is defined as the change in the measure of randomness in the reaction. It is represented as . Randomness of gaseous particles is more than that of liquid which is further more than that of solids.
For the given exothermic reaction:
As, number of gaseous particles on the product side is more than the number of gaseous particles on the reactant side. So, the entropy change is positive. Hence, is positive.
The above reaction is spontaneous. Thus, the Gibbs free energy will be negative.
For the given reaction:
The answer is 67 hope this helps!!