1. For the reaction of nitric oxide (NO) and oxygen to form nitrogen dioxide, if molecular oxygen is reacting at the rate of 0.00072 M/s, what is the rate (in M/s) of nitric oxide reacting?
2. For the reaction of nitric oxide (NO) and oxygen to form nitrogen dioxide, if molecular oxygen is reacting at the rate of 0.00697 M/s, what is the rate (in M/s) of nitrogen dioxide being formed?
1. For the reaction of nitric oxide (NO) and oxygen to form nitrogen dioxide, if molecular...
The reaction between nitric oxide (nitrogen monoxide) and oxygen gives nitrogen dioxide according to the stoichiometric equation. 2 NO(g) 02(g)2 NO2(g) 1. Write the rate law expected if the reaction was found to occur in a single step The reaction is observed to be complex with the following mechanism is proposed: 2 NO N202 N202 2 NO N202 +02 → 2NO2 k2 kı k. -1 2. Use the steady state approximation to obtain the expression for the formation of NO2....
Question 16 5 pts Nitrogen dioxide dissociates to form nitric oxide and oxygen 2 NO2)2 NO(g) + O2(8) What is value of the equilibrium constant for the reverse reaction if the equilibrium concentration of NO2 is 0.240 M, NO is 0.112 M, and O2 is 0.360 M at 33°C? 0108 0.0784
Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g) + O_2(g) 2 NO_2(g) What is K_c for the forward reaction if the equilibrium concentration of NO is 0.200 M, O_2 is 0.100 M, and NO_2 is 0.250 M at 25 degree C? 8.00 times 10^-2 6.41 times 10^-2 12.5 15.6
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
QUESTION 2 Colorless gas nitric oxide gas, NO, can react with oxygen to form the brown gas nitrogen dioxide, NO2, as shown below 2 NO(g)+ O2(g)-2 NO2(g) Suppose you wanted to carry out this reaction in the laboratory. You could filled one gas syringe with 100. mL of nitric oxide and another with 90. mL of oxygen gas. When you connected the syringes and mixed the gases, the reaction mixture changes to a brown color indicating the the reaction had...
the decomposition of nitric oxide to molecular nitrogen and oxygen as shown in the following equation occurs at high temperatures. when the reaction is at equilibrium kc= 0.640 If a sealed 1 L vessel is initially charged with 4.0 mol of NO gas, what is the concentration of NO at equilibrium?
Colorless gas nitric oxide gas, NO, can react with oxygen to form the brown gas nitrogen dioxide, NO2, as shown below: 2 NO(g) + O2(g) → 2 NO2(g). Suppose you wanted to carry out this reaction in the laboratory. You could filled one gas syringe with 100. mL of nitric oxide and another with 111. mL of oxygen gas. When you connected the syringes and mixed the gases, the reaction mixture changes to a brown color indicating the the reaction had...
QUESTION 1 (10) Nitric oxide reacts with oxygen to form nitrogen dioxide: 2NO(g) + O2(g) + 2NO2 (g) a) What is the Kc for the reaction if the equilibrium concentration of NO is 0.300 M, O2 is 0.200 M, and NO2 is 0.530 M at 25°C? b) What is the Kp for the same reaction? c) If the equilibrium re-establishes where [NO]=0.150 M and [02]-0.225 M, what is [NO2) at this point under the same temperature? 2(12) The equilibrium constant...
II Review Constants Peri Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2(g) + 2NO(g) + O2(g) Part A In a particular experiment at 300°C, NO2 drops from 0.0100 to 0.00750 M in 100 s. The rate of appearance of O2 for this period is M/s. X 2.5 x 10-3 OOOOO 5.0 x 10-3 5.0 x 10-5 2.5 x 10-5 1.3 x 10-5 Submit Request Answer
Nitrogen and oxygen gas react as high temperatures to form nitric oxide, a component of photochemical smog. Net reaction: the net reaction is N2 + O2 --> 2NO Proposed mechanism: O2 <====> 2O (fast, at equilibrium) N2 + O <-- --> NO + N (fast, not at equilibrium) N + O2 ----> NO + O (Slow) a.) Derive the rate law for the proposed mechanism. rate = ____________________________ b.) What is the initial rate law, when very little...