1)
Rate 1 = -{[N2O5]final – [N2O5]initial}/Time
= -(1.529 - 1.605) x 1012/1.25
= -(- 0.076) x 1012 / 1.25
= 6.08 x 1010 molecules/cm3s
Rate 2 = -{[N2O5]final – [N2O5]initial}/Time
= -(1.471 - 1.529) x 1012/1.25
= - (-0.058)x1012 /1.25
= 4.64 x 1010 molecules/cm3s
Rate 3 = -{[N2O5]final – [N2O5]initial}/Time
= -(1.323-1.368) x 1012/1.25
= -(-0.045 x 1012 / 1.25
= 3.60 x 1010 molecules/cm3s
Rate 4 = -{[N2O5]final – [N2O5]initial} / Time
= -(1.389 - 1.425) x 1012/1.25
= -(-0.036 x 1012 / 1.25 )
= 2.88 x 1010 molecules/cm3s
The average rate of the reaction is = ( Rate 1 + Rate 2 + Rate 3 + Rate 4 ) / 4
= ( 6.08 + 4.64 + 3.60 + 2.88 ) x 10 10 / 4
= ( 1.72 x 1011 ) / 4
= 4.3 x 1010 molecules/cm3s
Dinitrogen pentoxide (N2O5) decomposes as follows to nitrogen dioxide and nitrogen trioxide: N,o,()NO,(g)-No, (g) Calculate the...
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)...
Dinitrogen pentoxide (N205) decomposes as follows to nitrogen dioxide and nitrogen trioxide: N205(8) —NO2(g) +NO3(g) Calculate the average rate of the reaction between consecutive measurement times in the following table. Time (s) [N205] (molecules/cm3) 0.00 1.605x1012 1.35 1.521x1012 2.70 1.455x1012 4.05 1.401x1012 5.40 1.357x1012 3rd attempt Part 1 (1 point) Feedback See Periodic Table Express every answer to two significant figures. Rate 1 = 2.55 x 10 11 molecules/cms) Part 2 (1 point) * Feedback Rate 2 = molecules/(cmºs) Part...
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)...
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...
tried it twice and theyre both wrong :/ Dinitrogen pentoxide (N2O5) 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 following table. Time (s) [N205] (molecules/cm²) 0.00 1.705x1012 1.95 1.625x1012 3.90 1.563x1012 5.85 1.513x1012 7.80 1.473x1012 Express every answer to two significant figures. Rate 1 = -1.7 x 1010 molecules/(cm3.s) Part 2 (1 point) & Feedback Rate 2 = -1.6 x...
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?
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...
1A. The decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N2O5 2 NO2 + ½ O2 is first order in N2O5 with a rate constant of 4.10×10-3 min-1. If the initial concentration of N2O5 is 0.510 M, the concentration of N2O5 will be M after 402 min h 1B. The gas phase decomposition of phosphine at 120 °C PH3(g)1/4 P4(g) + 3/2 H2(g) is first order in PH3 with a rate constant of 1.80×10-2 s-1. If the...
2N_2O_5(g) rightarrow 4NO_2(g) + O_2(g) The reaction of dinitrogen pentoxide decomposed into nitrogen dioxide and O_2 is first-order and has a rate constant of k = 9.55 times 10^-4 s^-1 under a particular set of conditions. What is the concentration of N_2O_5 in this system after 10.0 min if [N_2O_5]_0 = 0.807 M? Did you use the equation that relates initial reactant concentration, rate Number constant, time elapsed, and reaction concentration at time t for a first-order reaction? Did you...