The activation energy is the amount of energy required to initiate a certain reaction. The activation energy may considered as an "energy barrier" that has to be overcome in order for a reaction to begin. If a reaction has a lower activation energy, then it will occur more easily and at a faster rate than a reaction with a higher activation energy. Therefore, the reason that reaction 1 is faster than reaction 2 is because it has a lower activation energy than reaction 2.
Answer:
90%
Step-by-step explanation:
Let R = 100
Since, Z = 30% of R
Therefore, Z = 30% *100 = 30
Since, W = 3Z
Therefore, W = 3*30 = 90
Percentage of W of R
First get the difference between the 2008 price and 1990 which is $4.02-$1.37= $2.65. Then the difference you've got which is $2.65, divide it to the current market price which is $4.02 to get the how many percentage it increased since then, $2.65/$4.02= 0.65920398 then multiply it to 100. It would be 65.92 or 66% if rounded off to whole number.
What you put is correct. A’B’C’D’ is what would be shown if you rotate ABCD 90 degrees clockwise
