The concentration of reactant A (in M) in a reaction of A → products was monitored as a function of time. The experimental data were plotted in three graphs of [A] versus time, ln[A] versus time, and 1/[A] versus time as shown. Determine the reaction order. Reaction order graph Not enough information to determine the reaction order.
Zero order
First order
Second order
Not enough information to determine the reaction order.
The concentration of reactant A (in M) in a reaction of A → products was monitored...
What data should be plotted to show that experimental concentration data fits a first-order reaction? ln(k) vs. Ea ln[reactant] vs. time ln(k) vs. 1/T 1/[reactant] vs. time [reactant] vs. time
Most of the time, the rate of a reaction depends on the concentration of the reactant. In the case of second-order reactions, the rate is proportional to the square of the concentration of the reactant. Select the image to explore the simulation, which will help you to understand how second-order reactions are identified by the nature of their plots. You can also observe the rate law for different reactions. In the simulation, you can select one of the three different...
Someone monitored a reaction by observing the time it took for the reactant concentration halve. It was observed that from the initial concentration of 0.01M to 0.005M, it took 10sec, and then from 0.005M to 0.0025M it took 20sec. What reaction order this reaction likely is? How do you make conclusion, please explain.
1)The rate law of a reaction is rate =k[X]³. The units of the rate constant areL mol-1 s-1mol² L-2 s-1mol L-1S-2L² mol-2 s-1mol L-1S-12)Given the following rate law, how does the rate of reaction change if the concentration of Z is tripled? Rate =k[X]³[Y]²[Z]⁰The rate of reaction will increase by a factor of136803)What data should be plotted to show that experimental concentration data fits a first-order reaction?1 / [reactant] vs. time[reactant] vs. timeln (k) vs. Ealn (k) vs. 1 / Tln [...
The following reaction was monitored as a function of time: A?B+C A plot of ln[A] versus time yields a straight line with slope ?4.5×10?3 /s . What is the value of the rate constant (k) for this reaction at this temperature?
The following reaction was monitored as a function of time: A→B+C A plot of ln[A] versus time yields a straight line with slope −4.5×10−3 /s . If the initial concentration of A is 0.240 M , what is the concentration after 240 s ?
5. For the hypothetical reaction A products, the concentration of A was monitored with time. 12.0 - y = 0.07580x + 10.00 11.5 MA) (1/1) 11.0 - 10.5 10.0 0 5 10 15 20 25 30 Time (s) Based on the graph above: What is the order of the reaction? 15 What is the rate constant for the decomposition of A? Is it possible for the y-intercept to be zero?
please show the work Consider the chemical reaction: NO + Cl2 → NOCI + CI This reaction is first order in each reactant and second order overall. To measure the rate constant, k, you decide to overload the amount of Cl2, at a concentration of 4 mol/L. The NO concentration used is much lower than this value. It is a good approximation to assume that the concentration of Cl2 does not change during the time that the reaction is studied,...
3. (10 pts) The progress of a reaction in aqueous solution was monitored by absorbance measurements of a reactant at various times: Time (s) 0 54 171 390 720 1010 1190 Absorbance 1.67 1.51 1.24 0.847 0.478 0.301 0.216 Tim 54 171 390 720 1010 Determine the order of the reaction and the rate constant.
2.) Calculate the Radius of the spinning mass based on the following data: 1.6 14 12 Mass 50.1g z 1.0 0.8 Linear mwz b m 0.00995 ± 1.6x10 b 0.0760 ± 0.0011 0.6 r1.000 0.4 0.2 0.0 20 40 60 8о 100 120 140 Angular Velocity-22 ((rad/s)2) 3.) If you plotted Centripetal force vs. w mstead, would this change your answer? Try it 1.4 1.2 1.0 0.8 Quadratic Awz Buz+C A 0.00983 9.4x10- B 0.00171± 0.0013 0.6 Mass 50.1g C...