The gas phase reaction between NO2 and F2 is first order in [NO2] and first order in [F2l. What would happen to the reaction rate if the concentrations of both reactants were halved with everything else held constant?a. It would decrease by a factor of 2.b. It would increase by a factor of 4.c. It would increase by a factor of 2. d. It would remain unchanged. e. It would decrease by a factor of 4.

e.It would decrease by a factor of 4.

Explanation:

first order in [NO2]

first order in [F2]

The rate is then given as;

Rate = k [NO2][F2]

where k = rate constant =  And is constant for a reaction.

Let's insert some dummy values (Any values work, just be consistent);

[NO2] = 2

[F2] = 2

K = 3

Rate = 3*2*2

Rate = 12

What would happen to the reaction rate if the concentrations of both reactants were halved with everything else held constant?

[NO2] = 2 / 2 = 1

[F2] = 2 / 2 = 1

K = 3

Rate = 3*1*1

Rate = 3

Comparing both rates (12 and 3); the correct option is;

e.It would decrease by a factor of 4.

answer is: c. the experiment shows that the red substance experienced a chemical change.

this is chemical change (chemical reaction), because two new substances are formed (metalig liquid and gas), the atoms are rearranged and the reaction is followed by an energy change.

this is example of chemical decomposition.

chemical decomposition (analysis) is the separation of a single chemical compound into its two or more elemental parts or to simpler compounds.  

chemical decomposition is opposite of chemical synthesis.