The reaction described by the equation O 3 ( g ) + NO ( g ) ⟶ O 2 ( g ) + NO 2 ( g ) has, at 310 K, the rate law rate of reaction = k [ O 3 ] [ NO ] k = 3.0 × 10 6 M − 1 ⋅ s − 1 Given that [ O 3 ] = 7.0 × 10 − 4 M and [ NO ] = 5.0 × 10 − 5 M at t = 0 , calculate the rate of the reaction at t = 0 .

Explanation:

Equation of the reaction:

O3(g) + NO(g) ⟶ O2(g) + NO2(g)

From the Rate Law:

R = k[O3][NO]

The order of NO is 1 and that of O3 is also 1, therefore order of reaction = 1 + 1

= 2

Given :

Concentration of O3, [O3] = 7.0×10^-4M

Concentration of NO, [NO] = 5.0×10^-5M

Rate constant, k = 3.0 × 10^6M^-1s^-1

R = 3.0×10^6 × 7.0×10^-4 × 5.0×10^-5

= 0.105 M/s

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

1.solid

2.carbon dioxide

3.helium