10) For 2NO+O2-2NO2, initial rate data are: NO] 0.010 0.010 0.030 M [O2] 0.010 0.020 0.020 M rate 2.5 5.0 45.0 mM/sec The rate law is Rate =k(NOMO2y: A)x=1,y-2 B) x = 2, y = 1 9x=0,y=2 D)x=2,y-2 E) x 1, y = 1 11) What is the rate-determining step for a reaction? A) The rate-determining step is the slowest elementary ste B) The rate-determining step is the fastest step in a reactio C) The D) The rate-determining step involves the largest number rate-determining step is a unimolecular reaction th are based on the reaction at equilibrium: C(s) + CO2(g)-2CO(g) ì¬" = +172.5 kJ/1 12) What is the effect on the position of equilibrium of de
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Related questions
1) The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 3.32 Ã10â10 sâ1 at 25°C. Calculate the rate constant at 58.3°C if the activation energy is 116 kJ/mol.
(Enter your answer in scientific notation.)answer
2)Given the same reactant concentrations, the reaction
CO(g) + Cl2(g) â COCl2(g)at 259°C is 272 times as fast as the same reaction at 147°
C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.
kJ/mol answer
3)For a certain reaction, the frequency factor A is 7.5 Ã109 sâ1 and the activation energy is 24.5 kJ/mol.
What is the rate constant for the reaction at 92°C
(Enter your answer in scientific notation.) answer
4)The rate constant of a first-order reaction is 3.25 Ã10â4 sâ1 at 350.°C. If the activation energy is 107 kJ/mol,
calculate the temperature at which its rate constant is 9.85 Ã10â4 sâ1.
5)The rate at which tree crickets chirp is 1.80 Ã102 per minute at 29°C but only 37.9 per minute at 6.5
°C. From these data, calculate the activation energy for the chirping process.
kJ/mol answer
6)Consider the following elementary step
X + 2Y âXY2
If the initial rate of formation of XY2 is 0.0076 M/s and the initial concentrations of X and Y are 0.38 Mand 0.64 M, what is the rate constant for the reaction?
Mâ2sâ1 answer
7)The activation energy for the decomposition of hydrogen peroxide is 59.0 kJ/mol. When the reaction is catalyzed by the enzyme catalase, it is 6.00 kJ/mol.
2H2O2(aq) â2H2O(l) + O2(g) |
Calculate the temperature that would cause the nonenzymatic catalysis to proceed as rapidly as the enzyme-catalyzed decomposition at 20.0°C. Assume the frequency factor, A, to be the same in both cases. Report your answer to 3 significant figures.
8)The activation energy (Ea) for the reaction
2N2O(g) â 2N2(g) + O2(g) ÎH
|
is 370.0 kJ/mol. What is the (Ea) for the reverse reaction?
kJ/mol answer