The reaction 2 NO(g) + O2(g) --> 2 NO2(g) is important in forming smog. Under certain conditions, the rate law for a the reaction is

rate = 4.0 x 10-3 1/M2*s * [NO]2* [O2]

What is the rate when [NO]=0.020 M and [O2]=0.035 M?

a.
5.6 x 10-2 M/s

b.
9.8 x 10-5 M/s

c.
9.8 x 10-8 M/s

d.
9.8 x 10-2 M/s

e.
5.6 x 10-8 M/s.

To find the rate of the reaction, we need to substitute the given concentrations of [NO] and [O2] into the rate law equation.

Rate = k[NO]^2 * [O2]

Where k is the rate constant. However, the value of the rate constant is not given.

Given: [NO] = 0.020 M and [O2] = 0.035 M

Substituting the given values into the rate law equation, we get:

Rate = k * (0.020 M)^2 * (0.035 M)

Rate = k * 0.0004 M^2 * 0.035 M

Rate = k * 1.4 * 10^-5 M^3

As the concentration units in the rate law are M^3, the rate will be in (M/s).

Now, to determine the numerical value of the rate, we need to know the value of the rate constant (k), which is not provided in the question. Therefore, we cannot calculate the specific rate given the information given.

Hence, the answer is not determinable with the information provided.

Can't you just plug in the numbers and solve it. The problem gives you the equation as well as the numbers. It's just a matter of punching in the numbers into the calculator.

rate = 0.004*(0.020)^2(0.035)
Solve for rate.