Let the rate law be:
Rate = k [NOBr]^x
From row 1:
Rate = k [NOBr]^x
1.62*10^-3 = k (0.0450)^x
From row 2:
Rate = k [NOBr]^x
7.69*10^-4 = k (0.0310)^x
Divide 1st equation by 2nd one
1.62*10^-3 / 7.69*10^-4 = (0.0450/0.0310)^x
2.11 = (1.45)^x
(1.45)^2 = (1.45)^x
So,
x = 2
The rate law is:
Rate = k [NOBr]^2
Put values from row 1
1.62*10^-3 mol.L-1.s-1= k (0.0450 mol.L-1)^2
K = 0.800 L.mol-1.s-1
Answer: b
QUESTION 6 2NOBr(g) → 2NO(g) + Br2(g) [NOB:](mol =) Rate (mol-1,-1) 0.0450 162 * 10-3 0.0310...
2NOBr(g) rightarrow 2NO(g) + Br2(g) [NOBr] (mol L^- 1) 0.0450 0.0310 0.0095 Rate (mol L^- 1 s^- 1) 1.62 times 10^-3 7.69 times 10^- 4 7.22 times 10^- 5 Based on the initial rate data above, what is the value of the rate constant? 27.8 L mol^-1 s^- 1 0.0360 s^- 1 0.800 L mol^- 1 s^- 1 0.0360 L mol^- 1 s^- 1 1.25 L mol^- 1 s^- 1
for the reaction 2NOBr(g)---- 2NO(g)+Br2(g) the rate
of the reaction -2.3 mol NOBr/L/h when the initial NOBr
concentration was 6.2 mol NoBr/L. what is the rate constant of the
reaction.
Please help:)
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