Question 5 What is the correct coefficient in the rate expression for nitrogen dioxide when it...
When dinitrogen pentoxide reacts with nitrogen dioxide, the products are nitrogen monoxide and molecular oxygen. If 50.00 g of dinitrogen pentoxide reacts with excess molecular oxygen at 28.0oC and the products are collected in a 700.0 L tank, what is the partial pressure of each gas and what is the total pressure in the tank assuming the reaction goes to completion? The unit for pressure should be in atm. NOTE: YOU MUST USE MOLE FRACTIONS FOR THE PARTIAL PRESSURES
Question 6 1 pts Dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen, all species are gaseous. Given 19.19 g of dinitrogen pentoxide, how many grams of oxygen will be produced when the reaction goes to completion? No new data to save. Last checked at 9:15am Submit Quiz
Question 6 1 pts Dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen, all species are gaseous. Given 19.19 g of dinitrogen pentoxide, how many grams of oxygen will be produced when the reaction...
02 Question (4 points) Dinitrogen pentoxide (N2O) decomposes as follows to nitrogen dioxide and nitrogen trioxide: N205(8) ► NO2(g) + NO3 (8) Calculate the average rate of the reaction between consecutive measurement times in the fbllowing table. Time (s) (N2O5] (molecules/cm) 0.00 1.605x1012 1.45 1.526x1012 2.90 1.465x1012 4.35 1.416x1012 5.80 1.377x1022 1st attempt 3 OF S QUESTIONS COMPLETED < 02/05 > Part 1 (1 point) Express every answer to two significant figures. Rate 1 = molecules/(cmºs) Part 2 (1 point)...
4) At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N2O3(g) - ANO, (2) + O2(g) Write the general rate expression using all chemical species: 5) Ar elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N,Os(8) ANO, (g) + O, (g) When the rate of formation of NO, is 5.5 x 10-M/s, the rate of decomposition of No, is M/s. 6) . A[NH 1 = a[Nal = +2H2] = + Write the balanced equation for a...
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.81 h at 25 ?C . If a 1.7-L reaction vessel initially contains 760 torr of N2O5 at 25 ?C , what partial pressure of O2 is present in the vessel after 205 minutes?
02 Question (4 points) Dinitrogen pentoxide (N2Os) decomposes as follows to nitrogen dioxide and nitrogen trioxide: N,0(8) NO,(8) + NO3(8) Calculate the average rate of the reaction between consecutive measurement times in the following table. Time (s) [N,Os) (molecules/cm) 0.00 1.805x1012 1.65 1.728x1012 3.30 1.669x1012 1.622x1012 6.60 1.585x1012 4.95 Part 1 (1 point) Express every answer to two significant figures. Rate 1 = molecules/(cm’s) Part 2 (1 point) Rate 2 = molecules/cms) Part 3 (1 point) Rate 3 = molecules/(cms)...
Nitrogen dioxide can react with ozone to form dinitrogen pentoxide and oxygen: 2NO2(g) + O3(g) → N2O(g) + O2(g) a) Based on the above information, write the two-step mechanism for this reaction b) Identify and write the rate law for this reaction:
02 Question (4 points) Dinitrogen pentoxide (N2Os) decomposes as follows to nitrogen dioxide and nitrogen trioxide: N,05(8) ► NO,(8) + NO,(8) Calculate the average rate of the reaction between consecutive measurement times in the following table. Time (s) IN 20s) (molecules/cm3) 0.00 1.405x1012 1.344x1012 1301x102 1270x102 1.249x102 IN E 1st attempt Part 1 (1 point) W See Pe Express every answer to two significant figures late 1 molecules/(cms) Part 2 (1 point) Rate 2- molecules (cm.) 1st attempt Part 1...
Nitrogen dioxide can react with ozone to form dinitrogen pentoxide and oxygen: 2NO2(g) + O3(g) → N2O(g) + O2(g) a) Based on the above information, write the two-step mechanism for this reaction: b) Identify and write the rate law for this reaction: c) Which step above is the rate determining step and why?
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?