he decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 K is 4.5  10-2 s-1   (a) If we begin with an initial SO2Cl2 pressure of 340. torr, what is the pressure of this substance after 70. s? (b) At what time will the pressure of SO2Cl2 decline to one half its initial value?   By what factor will the pressure of sulfuryl chloride decrease after 4 half lives? Note: The answer wants this value: (340. torr)/value = final pressure after decay

As described in Exercise 14.41, the decomposition of sulfuryl chloride 1SO2Cl22 is a first-order process. The rate constant for the decomposition at 660 K is 4.5 * 10-2 s-1. (a) If we begin with an initial SO2Cl2 pressure of 450 torr, what is the partial pressure of this substance after 60 s?

The decomposition of sulfuryl chloride, SO2Cl2, to sulfur dioxide and chlorine gases is a first-order reaction. It is found that at a certain temperature, it takes 1.43 hours to decompose 0.0714 M  to 0.0681 M. What is the rate constant for the decomposition?

The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the following equation: OCl–(aq) + I–(aq) → OI–(aq) + Cl–(aq) The rate law for this reaction is Rate = k [I-][OCl-]/[OH-]. The overall reaction order and the order with respect to OH- are?

The decomposition of sulfuryl chloride (S0₂Cl₂) is a first-order process. The rate constant for the decomposition at 660 K is 4.5 x 102 ¹ (a) If we begin with an initial 50₂Cl₂ pressure of 335 torr, what is the pressure of this substance after 76 s? torr (b) At what time will the pressure of 50₂Cl₂ decline to one fourth its initial value? By what factor will the pressure of sulfuryl chloride decrease after 4 half lives? Note: The answer wants this value: (335 torr)/value final pressure after decay value

The first-order rate constant for the decomposition of N205, given below, at 70°C is 6.82 10-3 s. Suppose we start with 0.0200 mol of N205(g) in a volume of 5.0 L. 2 N205(g) → 4 NO2(g) + O2(g) (a) How many moles of N205 will remain after 1.5 min? mol (b) How many minutes will it take for the quantity of N205 to drop to 0.005 mol? min (c) What is the half-life of N205 at 70°C? min

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?

Acetaldehyde decomposes when heated to yield methane and carbon monoxide according to the equation, CH3CHO(g) → CH4(g) + CO(g) Based on the experimental data provided below: (a) Determine the rate law (b) Determine the rate constant (c) Determine the half-life, in hours, for the decomposition [CH,CHO] (mol/L) -d[CH,CHO]/dt (mol/L-s) 1.75 X 103 2.06 X 1011 3.50 X 10-3 8.24 X 10-11 7.00 X 10-3 3.30 X 10-10

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A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: (1) H₂O2(g) →>> 2OH(g) (2) H₂O2(g) + OH(g) → H₂O(g) + HO₂(g) (3) HO₂(g) + OH(g) → H₂O(g) + O₂(g) If the rate law for the reaction is first order in H₂O2, which step in the mechanism is the rate-determining step? O Step 1 O None of the steps O Step 3 O Impossible to determine Steps 1 and 2 O All of the steps O Step 2 Hint: The slowest step in a mechanism determines the rate law. From each elementary reaction we can write a rate-law expression. Submit Question