Question

Use the References to access important values if needed for this question. The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution NH, NO 2 Ho 2req 780 780 1.56 1.56 6.56 102 1.54 10-5 07 105 3.07 10-5 6.13 10 0.131 56x10 131 ts 2req Complete the rate law for this reaction in the box below Use the form kIAl(B, where '1' is understood for m or n and concentrations taken to the zero power do not appear: Don't enter 1 for m orn pts From these data, the rate constant is M11 Submit Aswe Retry Entire Groug 9 more

help it this 3 questions please

Answer 1

1.

Do, (1) / (2)

1.54 * 10^-5 / (3.07 * 10^-5) = (6.56 * 10^-2 / 0.131)ⁿ

0.502 = (0.501)ⁿ

n = 1

Therefore, order with respect to NO₂^- = 1

Now do ((1) / (3)

1.54 * 10^-5 / (3.07 * 10^-5) = (0.780 / 1.56)^m

0.502 = (0.5)^m

So, m = 1

Therefore, order with respect to NH₄⁺ = 1

Over order of reaction = 1 + 1 = 2

Rate law expression can be written as,

Rate = k[NH₄⁺][NO₂^-]

From (1)

1.54 * 10^-5 = k(0.780)(6.56 * 10^-2)

k = 3.01 * 10^-4 M^-1s^-1