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kinds of kinds Consider the second-order reaction: 2HI(g) H₂(g) +1₂(g) Use the simulation to find the initial concentration [HI], and the rate constant & for the reaction. What will be the concentration of HI after t=5.45x10¹0s ( [HI],) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. ▸View Available Hint(s) 10 ΑΣΦΑ HI, - ? mol

kinds of kinds Consider the second-order reaction: 2HI(g) H₂(g) +1₂(g) Use the simulation to find the initial concentration [HI], and the rate constant & for the reaction. What will be the concentration of HI after t=5.45x10¹0s ( [HI],) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. ▸View Available Hint(s) 10 ΑΣΦΑ HI, - ? mol

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 25E: Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following...
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t of the time, the rate of a reaction depends on the centration of the reactant. In the case of second-order ctions, the rate is proportional to the square of the centration of the reactant. ect the image to explore the simulation, which will help you to derstand how second-order reactions are identified by the ture of their plots. You can also observe the rate law for ferent reactions. [HI] moll 0.5 10 15 time, 10s Plot [HI] vs time O Plot In[HI] vs. time O Plot 1(HI) vs. time 2.0 25 concentration, moll 2HI Rate law: KHI k-64-10°1(mol-s) at 500 K Initial rate-1.6-10 moll-s) 281-H₂+1₂ Start In the simulation, you can select one of the three different kinds of plots. You may use the Start, Stop, and Reset buttons to obronie th
Transcribed Image Text:t of the time, the rate of a reaction depends on the centration of the reactant. In the case of second-order ctions, the rate is proportional to the square of the centration of the reactant. ect the image to explore the simulation, which will help you to derstand how second-order reactions are identified by the ture of their plots. You can also observe the rate law for ferent reactions. [HI] moll 0.5 10 15 time, 10s Plot [HI] vs time O Plot In[HI] vs. time O Plot 1(HI) vs. time 2.0 25 concentration, moll 2HI Rate law: KHI k-64-10°1(mol-s) at 500 K Initial rate-1.6-10 moll-s) 281-H₂+1₂ Start In the simulation, you can select one of the three different kinds of plots. You may use the Start, Stop, and Reset buttons to obronie th
to kinds of kinds ing the s for Part B Consider the second-order reaction: 2HI(g)→H₂(g) +12(g) Use the simulation to find the initial concentration [HI], and the rate constant & for the reaction. What will be the concentration of HI after t = 5.45x10¹0s ( [HI]) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. View Available Hint(s) - Submit 196) ΑΣΦΑ Part C Complete previous part(s) Part D Complete previous part(s) ? mol L
Transcribed Image Text:to kinds of kinds ing the s for Part B Consider the second-order reaction: 2HI(g)→H₂(g) +12(g) Use the simulation to find the initial concentration [HI], and the rate constant & for the reaction. What will be the concentration of HI after t = 5.45x10¹0s ( [HI]) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. View Available Hint(s) - Submit 196) ΑΣΦΑ Part C Complete previous part(s) Part D Complete previous part(s) ? mol L
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