Answer Happy

Here is a graph of the pressure of oxygen O₂) in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the tabl below. atm D 30+ 25 24.513 20 15- 10- 5- 0 50 100 150 seconds Is O₂ being created or destroyed by the chemical reaction? 200 250 created O destroyed 300 X Oneither created nor destroyed ☐ x10 00 9 ロ･ロ
If O₂ is being created or destroyed, what is the rate at which it is being created or destroyed 80 seconds after the reaction starts? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. If O₂ is being created or destroyed, what is the average rate at which it is being created or destroyed during the first 80 seconds of the reaction? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. Oneither created nor destroyed -0.15 -0.16 atm S atm S ?
Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 1.41M 1.48M 0.217M/s 1.41M 4.29M 2.62M 1.48M Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k [₂] [¹¹₂] -1 -1 0.629 M/s 0.749 M/s k = 0.10 M S 0x10 X Ś ?
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0388 s 2C1₂O5 (g) → 2Cl₂ (g) +50₂ (g) - Suppose a vessel contains C1₂O5 at a concentration of 0.410M. Calculate the concentration of C1₂O5 in the vessel 22.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. 41 x 10 ²IM x10 ?