The reaction 2NO(g)+O2(g)→2NO2(g) is second order in NO and first order in O2. When [NO]= 4.5×10−2 M and [O2]= 3.7×10−2 M , the observed rate of disappearance of NO is 9.9×10−5 M/s . What is the rate of disappearance of O2 at this moment?
The reaction 2NO(g)+O2(g)→2NO2(g) is second order in NO and first order in O2. When [NO]= 4.5×10−2...
2. (10 pts) Consider the following second-order reaction: 2NO2(g) + 2NO(g)+O2(g) The rate constant is 0.54 M-15-1, at 300 °C. How long would it take for the concentration of NO2 to decrease from 0.62M to 0.28M?
9. The reaction 2NO +O2 → 2NO2 is believed to occur by the following mechanism: 2NO ↔ N2O2 N2O2 + O2 → 2 NO2 a. Assume N2O2 to be in a steady state and derive the rate equation for the overall reaction. b. Under what condition does the rate equation reduce to second order kinetics in NO and first order kinetics in O2 at the same time?
Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2→2NO+O2 In a particular experiment at 300 ∘C, [NO2] drops from 0.0256 to 0.00889 M in 383 s . The rate of disappearance of NO2 for this period is ________ M/s. 1) 4.36×10−5 2) −9.01×10−5 3) 8.73×10−5 4) 2.29×104 5) 2.18×10−5
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g)2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH∘ΔH∘ and ΔS∘ΔS∘ do not change too much within the give temperature range.) 1) 713 2) 852
The following data were collected for the rate of disappearance ofNO in the reaction 2NO(g) + O2 --> 2NO2(g) : Experiment [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.0126 0.0125 1.41 x 10-2 2 0.0252 0.0125 5.64 x 10-2 3 0.0252 0.0250 1.13 x 10 -1 (a) What is the rate law for the reaciton? (B) What are teh unitsof the rate constant? (c) What is the average value of the rateconstant calculated form teh three data sets? (d)...
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature K 400 1.9x10^7 425 2.5x10^6 465 1.6x10^5 515 8.8x10^3 600 2.0x10^2 Use the data to find ΔrS∘ΔrS∘ for the reaction. (answer in J K-1 mol-1) The answer is NOT 158
2NO2(g) → 2NO(g) + O2(g) Describe the reaction and the importance of the molecules involved. Describe what needs to happen on a molecular level in order for the reaction to take place.
The equilibrium constant KcKc for the reaction 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) is 6.9×1056.9×105 at 500 KK. A 5.0 LL reaction vessel at 500 KK was filled with 0.052 molmol of NONO, 1.1 molmol of O2O2, and 0.90 molmol of NO2NO2. Part A What is the value of QcQc? Express your answer to two significant figures.
4. . The reaction 2NO(g) + O2(g) → 2NO2(g) has the following rate law: Rate = k[O2][NO]2 . If the concentration of NO is reduced by a factor of two, the rate will __________
2- For the reaction 2NO(g) + O2(g)2NO2(g) H° = -114.2 kJ and S° = -146.5 J/K The equilibrium constant for this reaction at 289.0 K is ---------- . Assume that H° and S° are independent of temperature.