The following results have been obtained during the kinetic studies of reaction: 2NO + 2H_2 → N_2+2H_2O Expt. \frac{-d[NO]}{dt} mol L^{-1}s^{-1} [NO] mol L^{-1} [H_2] mol L^{-1} 1. 4.8 × 10^{-5} 1 × 10^{-2} 1 × 10^{-3} 2. 43.2 × 10^{-5} 3 × 10^{-2} 1 × 10^{-3} 3. 86.4 × 10^{-5} 3 × 10^{-2} 2 × 10^{-3} The rate Law is:

Correct Answer is : −d[NO]dt = k [NO]2[H2]

\frac{-d[NO]}{dt} = k [NO]^2[H_2]

\frac{-d[NO]}{dt} = k [NO]^2[H_2]^{1/2}

\frac{-d[NO]}{dt} = k [NO][H_2]^2

\frac{-d[NO]}{dt} = k [NO][H_2]

TS EAMCET 03 May 2019 Shift 2 Solved Paper

Section: Chemistry

Question : 146 of 160

Marks: +1, -0

The following results have been obtained during the kinetic studies of reaction:
2NO + 2H2 → N2+2H2O

Expt.

−d[NO]

mol L−1s−1

[NO]
mol L−1

[H2]
mol L−1

4.8 × 10−5

1 × 10−2

1 × 10−3

43.2 × 10−5

3 × 10−2

1 × 10−3

86.4 × 10−5

3 × 10−2

2 × 10−3

The rate Law is:

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