Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0025 M-s¯¹: 2 HI (g) → H₂(g) +1₂ (8) Suppose a 500. mL flask is charged under these conditions with 450. mmol of hydrogen iodide. How much is left 90. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. 0 X x10

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of ·0.0040Ms−1:2HI(g)→H2(g)+I2(g)   Suppose a 300.mL ⁢ flask is charged under these conditions with  500.mmol of hydrogen iodide. After how much time is there only  250.mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

Consider this reaction: 2H,PO, (aq)→ P,0, (aq) + 3H,0 (aq) At a certain temperature it obeys this rate law. rate = (14,5 M)[H,PO.] Suppose a vessel contains H,PO at a concentration of 1.17 M. Calculate how long it takes for the concentration of H,PO to decrease by 84.0%. You may 4 assume no other reaction is important. Round your answer to 2 significant digits.

Deducing a rate law from the change in concentration over time A chem raduate student is studying the rate of this reaction: 2N,05 (g) → 2N,0,(g)+O, (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds: time (seconds) N,0s] 0.0300 M 1.0 0.0114 M 2.0 0.00707 M 3.0 0.00511 M 4.0 0.00401 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k I %3D x10 Calculate the value of the rate constant k. k = 0 Round your answer to 2 significant digits. Also be sure vour answer has the correct unit svmbol. Explanation Check 2021 McGraw-Hill Education. II

Consider the following balanced chemical equation: H2O2 (aq) + 3 l"(aq) + 2 H* (aq) → l3 (aq) + 2 H2O (1) In the first 32.7 seconds of the reaction, the concentration of H2O2 decreased from 1.5 M to 0.72 M. What is the average reaction rate over this time interval (in mol L-1 s-1)? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:

The rate of the reaction NO2+ CO - NO + CO2 depends only on the concentration of nitrogen dioxide, NO2. The following data were collected. time (s) [NO] (M) 0.500 1.20 x 10 0.444 3.00 x 10 0.381 4.50 x 10 0.340 9.00 x 10 0.257 1.80 x 10 0.174 When entering values in scientific notation follow this format: 6.022 x 1023 would be 6.022e23 (no spaces) 1. Using graphical analysis (Google Sheet et) determine the overall reaction order. (0.1.2) Be sure to upload a screenshot copy of the the Google sheet for question 2 in the next question box. 2 Determine the value of the rate constant for the reaction (do not round answer). 3. Calculate the [NO2l, at 2:40 x 10 s. (show answer to 3 places after the decimal) 182 4. Determine the t, for the reaction. (round answer to the whole number)

Consider this reaction: H,CO, (ag) – H,0 (aq) + CO, (ag) At a certain temperature it obeys this rate law. rate = (9.70 x 10-4s)H,co,] Suppose a vessel contains H,CO, at a concentration of 0.470 M. Calculate the concentration of H,CO, in the vessel 680. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. x10

Under certain conditions the rate of this reaction is zero order in hydrogen lodide with a rate constant of 0.0038 M's ': 2 HI(g) H,(g)+1,(g) Suppose a 4.0L flask is charged under these conditions with 100, mmol of hydrogen lodide. After how much time is there only 50.0 mmol left? You may assume no other reaction Is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

Consider this reaction: 2HI (g) → H₂ (g) + 1₂ (g) At a certain temperature it obeys this rate law. rate = (0.00315 M¹-s¯¹) [HI] ² S olo Suppose a vessel contains HI at a concentration of 1.16M. Calculate the concentration of HI in the vessel 970. seconds later. You may assume no other reaction is important. Ar Round your answer to 2 significant digits. M x10 X Ś ?

Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0032 M's : 2 NH, (g) → N2 (g) +3 H, (g) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of ammonia. How much is left 10. s later? You may assume no other reaction is important. olo Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. Ar