or this reaction. H,CO, (aq) H,0 (ag)+CO, (aq) She fills a reaction vessel with H,C0, and measures its concentration as the reaction proceeds. Here's a graph of her data: 15- 05-- * (seconds) Use this graph to answer the following questions What is the half life of the reaction? 1/2 0 Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in H,CO,. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of H,CO, in the engineers reaction vessel after 1.20 seconds have passed. Assume no other reaction is important, and continue to [#,co.] = M H.CO assume the rate is first order in H. CO,. H,CO,. 31 Round your ansver to 2 s gnificant digits. ((*0)°H]

Subject- chemistry

Determine the rate of formation of I3− if the initial concentration of I− was 0.5583 M and decreased to 0.4566 M after 0.3335 hours. Use the reaction below.3I−(aq)+ S2O82−(aq) ↔ I3−(aq) + 2SO42−(aq)

A chemical engineer is studying the rate of this reaction. 2N,0, (g) → 2N,O4g)+O2 (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds. Here's a graph of his data: 2 1.5 - 0.5 0. 0.2 0.4 0.6 0.8 1.2 t (s) (x) [°o°n]

The scenes depict three initial reaction mixtures for the reaction of A (blue) and B (yellow). The initial rate, -d[A]/dt (in mol/Is), is shown, with each sphere representing 0.010 mol and the container volume at 0.50 L. Initial rate is given below the pictures. What is the rate constant, k? Enter a number. Copyright © McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of McGraw-Hil Education. I 10.0 п 16.0 ш 16.0

Determine the average rate of change of B from t = 0 s to = 362 s. A → 2B rate = M/s Time (s) 0 181 362 Concentration of A (M) 0.720 0.425 0.130

The rate of a reaction is monitored by measuring the number of moles of product that form per liter per second. The data obtained are listed in the table below. Using this data, mathematically determine the order with respect to each reactant, the overall order of the reaction, determine the rate constant, k, with units, and write the complete rate law. Experiment [X], M [Y], M Rate, Msec-1 1 0.0500 0.0850 0.643 2 0.0300 0.0850 0.386

Determine the order of the reaction and the value of the rate constant.  Having trouble figuring out how to use the half life's to figure out the order of the reaction.

A particular reactant decomposes with a half-life of 121 s when its initial concentration is 0.354 M. The same reactant decomposes with a half-life of 239 s when its initial concentration is 0.179 M. Determine the reaction order. 01 What is the value and units of the rate constant for this reaction? Units 0.17 Enter numeric value TOOLS x10