A reaction involving NO_2 proceeds according to the rate law rate = k[NO_2]^3. W

Question

A reaction involving NO_2 proceeds according to the rate law rate = k[NO_2]^3. What is the value of the rate constant for this reaction if the rate of the reaction is 1.07 times 10 M/s when the [NO_2] = 0.119 M? Enter your answer to the hundredths place. What are the units of the constant for the reaction in Question.? S^-1 M/s 1/M-s 1/M^2-s Technetium-99m (Tc) is commonly used as a radioisotope for medical purposes. The "m" denotes it as metastable, since its nucleus is in an excited state, which relaxes to its ground nuclear state by emitting gamma radiation with a half life of 6.01 hours. For a 1.00 mu g sample of Tc, how many hours will it take the sample to decompose to 0.354 mu g? Enter your answer to the hundredths place. For what order reaction (0, 1, or 2) will a plot of concentration versus time be linear? The reaction of stratospheric ozone with chlorine radicals has an activation energy of 39.1 kJ/mol. If the rate constant for the reaction is 196.7 1/M-s at -65.0 degree C, at what temperature, in Kelvin, will the rate constant be doubled? Enter your answer to the ones place. What is the molecularity (unimolecular, bimolecular, or termolecular) of the elementary reaction H_2g + 2l(g) rightarrow 2HI(g)? **Questions 14-15 refer to the reaction mechanism given below** Step 1: H_2Og) + ICI(g) rightarrow HCI(g) + HI(g) slow Step 2: HI(g) + ICI(g) HCl(g) + I_2(g) fast Overall: H_2(g) + 2ICl(g) 2HCI(g) + I_2(g) What is the rate law predicted by this mechanism? Rate = k[K_2][ICI] rate = k[HI][ICI] rate = k[H_2][ICI]^2 rate = k [HCI]^2[I_2]/[H_2][ICI]^2 In this mechanism, HI can best be described as a(n): Catalyst Transition State Activated Complex Intermediate

Explanation / Answer

12.

k1 = 196.7 M-1s-1

k2 = 2x196.7 M-1s-1

T1 = 208 K

R = 8.314JK-1mol-1

Ea = 39.1 kJ/mol = 39100 J/mol

ln(k2/k1) = Ea/R x (1/T1 - 1/T2)
ln(2) = Ea /8.314 x (1/208 - 1/T2 )
0.693= (39100 / 8.3145)x(4.80x 10-3 -1/T2)

T2 = 214.5K

13.

The elementary step determines the molecularity of the reaction.

So the molecularity of the given reaction is trimolecular in nature

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