Data in the table were collected at 540 K for the following reaction: CO + NO2 = CO2 + NO Determine the reaction order with respect to each reactant. Order with respect to CO:   Order with respect to NO2

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 hh at 25 ∘C∘C. If a 1.7 −L−L reaction vessel initially contains 760 torrtorr of N2O5N2O5 at 25 ∘C∘C, what partial pressure of O2O2 will be present in the vessel after 230 minutes?

The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic…

The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N2O5 and first order overall.  The rate constant for the reaction at 70.oC is 6.82x10-3 s-1.  The reaction is started with 0.300 mol of N2O5 in a 0.500L container. How many minutes will it take for the concentration of N2O5 to drop to 0.145M?

The first-order rate constant for the decomposition of C2H5Cl, C2H5Cl(g)  C2H4(g) + HCl(g) at 27 oC is k = 7.27e-30 s-1. Suppose we start with 0.0845 mol of C2H5Cl in a volume of 4.9 L. How many moles of C2H5Cl will remain after 1.24e+27 min?

How do you find the order for [O2]?

6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179

Data in the table were collected at 540 K for the following reaction: CO(g) + NO₂(g) → CO₂ (g) + NO(g) Initial concentration (mol/L) [CO] 5.1 × 10-4 5.1 x 10-4 5.1 x 10-4 1.0 × 10-³ 1.5 × 10-³ [NO₂] 0.35 × 10-4 0.70 × 10-4 0.18 × 10-4 0.35 × 10-4 0.35 × 10-4 Initial rate (mol/L. h) 5.0 × 10-8 1.0 × 10-7 2.6 × 10-8 9.8 × 10-8 1.5 × 10-7

The decomposition of ethyl chloride, CH3CH2Cl, follows the rate law: Rate = k[CH3CH2Cl]. At 550°C, k = 3.2 x 10-2 sec-1. What is the half-life for this reaction? What was the initial concentration of ethyl chloride if after one minute, 0.01 M remains?

At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.75Ms H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.130M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.0286 M. You may assume no other reaction is important. Round your answer to 2 significant digits. X ? S