Question

Some measurements of the initial rate of a certain reaction are given in the table below. N2] H] Initial rate of reaction 1.70 M 1,05 M 6.00 x 109 M's 0.676 M 1.05 M 9.49 x 10 m/s 1.70 M 0.495 M 1.33 x 104 m/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol rate = k = 0 5 ?

Answer 1

OB [Na] [ra] Initi ilms 1.7M 1.osm I 6X 10.676m 1.05m 9.49x13 Liam l 0-495m 11:33x10 Rate= k [~ 7² [ ] k- Rate Constant n- Order of Reaction with to respect, toN. y- Order of Reaction with respect to the Now, different Values of [~2] a [kg] we have different rates, so, I 6x10" = x [77 (los L a This is written from the first row of data in the table. [ 9.49 810 k[o: 6767 1.053 - (2) from the second row or Data Teacher's Signatur,

| 1-33x10" = K[73² [0.495] - (3 Dividing Equation 1 with 2, 6x109 KX [1-77°C1.0539 4.49 X103 = KX [0.676] [105] 9.90 => 163 = [05157" 5 m2] (approximately) Dividing Equation 1 with 3. Grio" kx[32*x [1-osa 7. 33 Xis**, *x [i*t* x [279577 >> Y512 Poss Fasva fondo] Teacher's Signature !

y=2 (approximately) so, Rate Equation = Rate Law l Rate= k [m] x [x2] I when Rate = 6X100 m [Na]= 1.7m, [2] = 105m 1So, 6x10 k (1.73** (10532 I kao 18831 mist In 3 significant digits, - Rate Constantz 18800 m s'