Explanation :
1)
half life at starting concentration is 1.81 = 663 s
half life at starting concentration is 0.905 = 1327 s
2)
average delta (1 / N2O) / delta t = 1/ 663 [1 / 0.905 - 1 / 1.81]
= 8.33 x 10^-4 M-1 s-1
In a study of the decomposition of nitrous oxide at 565 °C N20(g) N2(g) + %...
In a study of the decomposition of nitrous oxide at 565 °C N20(g)N2(g) + 2O2(g) the following data were obtained: [N2O], M 0.400 0.100 0.800 0.200 |1.61x103 seconds 1.13x104 4.82x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.800 M is 1.61x10^3 s and when the starting concentration is 0.400 M is 3.21x10^3 S. (2) м1s-1 The average A(1/[N2O]) / At from t = 0 s...
The decomposition of nitrous oxide at 565 °C N20() -N2(g) + O2() is second order in N, with a rate constant of 1.10X10's! If the initial concentration of N20 is 1.05 M, the concentration of N O will be Mafter 2.74x10 seconds have passed. Submit Answer Try Another Version 3 item attempts remaining In the laboratory you are asked to make a 0.506 m chromium(II) nitrate solution using 315 grams of water. How many grams of chromium(II) nitrate should you...
The decomposition of nitrous oxide at 565 °C N2O(g)----> N2(g) + ½ O2(g) is second order in N2O. In one experiment, when the initial concentration of N2O was 0.790 M, the concentration of N2O dropped to 0.103 M after 5.21×10^3 seconds had passed. Based on these data, the rate constant for the reaction is _____________ M-1 s-1.
the Weferescn to wcerss For the decomposition of nitrous oxide at 565 *C the following data have been obtained ate L and Apply INO, M The average rate of disappearance of N,O over the time period fromt-18.4sot-368s is 7 more group attempts remaining Retry Entire Group Submit Answer T/12 groups Due Agr 22 at 11:00 PM 8 6 5 4 3 2
The second-order rate constant has been measured at different temperatures for the decomposition of nitrous oxide (N20) into a nitrogen molecule and an oxygen atom. M T(°C) 1.87 x 10 3600.0 0.0113 .0569 0.244 50.0 00.0 50.0 Determine the activation energy for the reaction. mol
In a study of the decomposition of ammonia on a platinum surface at 856 °C NH3--------->1/2 N2 + 3/2 H2 the following data were obtained: [NH3], M 1.26×10-2 6.30×10-3 3.15×10-3 1.58×10-3 seconds 0 1000 1.50×103 1.75×103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.26×10-2 M is s and when the starting concentration is 6.30×10-3 M is s. (2) The average rate of disappearance of NH3...
In a study of the gas phase decomposition of nitrosyl chloride at 400 K NOCl(g)-NO(g) + ½ Cl2(g) the following data were obtained: [NOCI], M 5.48x10-2 2.74x10-2 1.37×10-2 6.85x10-3 seconds 3.80x104 1.14x10 2.66x105 Hint: It is not necessary to graph these data. The observed half life for this reaction when the starting concentration is 5.48×10-2 M is s and when the starting concentration is 2.74x10 M is S. Ms The average Δ(1/[NOCl) At from t-0 s to t-3.80x10" s is...
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...
Nitrous oxide (N20) is produced from ammonia nitrate under conditions such that 2000 kg of NH4NO3 produce 700 kg of N20. The equation for the reaction is: Atomic weight ofN is 14 g mol. O is 16 g mol. H is g mol-1 a) Calculate the percent conversion of NH4NO3 b) Calculate the percent yield on a mass basis. c) Calculate the percent yield on a mole basis. [2 marks] [1 mark] [1 mark]
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration of NOBr was followed as a function of time. It was found that a graph of 1/[NOBr] versus time in seconds gave a straight line with a slope of 1.27 m?s and a y-intercept of 3.98 M? Based on this plot, the reaction is order in NOBr and the rate constant for the reaction is M?? In a study of the decomposition of hydrogen...