![A reaction: A. has been studied at 25°C. Shown below are the experimental data. 1.04 0.667 0.565 These data are plotted three different ways, below, as [A] vs t, In[A] vs t and 1/[A] vs t. Use this information to calculate a value for the rate constant, k, and the initial concentration of A, [Alo to 3 significant figures ime () ime(s time (s) Submit Answer Incorrect. Tries 1/2 Previous Tries [A]0 (M) = Submit Answer Tries 0/2](http://img.homeworklib.com/questions/96f69130-2bee-11ec-a35a-bb798ed18e57.png?x-oss-process=image/resize,w_560)
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A reaction: A. has been studied at 25°C. Shown below are the experimental data. 1.04 0.667...
Find the rate constant and the initial concentration I know it's second order, just have no...
Find the rate constant and the initial concentration
I know it's second order, just have no clue how to find K from
this data, or what the initial concentration is. It also says that
the reaction is A -> C
has been studied at 25°C Shown below are the experimental data time (s) [A] (M 1.03 0.811 6 0.669 8 0.569 0.495 10 These data are plotted three different ways, below, as [A] vs t, In[A] vs t and 1/[A]...
At a certain temperature, the half-life of the first order decomposition of phenol (shown below) is...
At a certain temperature, the half-life of the first order decomposition of phenol (shown below) is 1.54 hr phenol cyclopentadiene carbon monoxide Answer the following questions about the decornposition of phenol and report all answers to three significant figures. 1. If the initial concentration of phenol is 8.73×10 2 M, calculate the time in hr required for the concentration o phenol to decrease to 50.3 % of the initial concentration. Submit Answer Tries 0/3 2. Tf the initial concentration of...
Calculate Reaction Rates From Experimental Data Question Given the data below of the concentration of compound...
Calculate Reaction Rates From Experimental Data Question Given the data below of the concentration of compound A for the reaction A > B, what is the average rate of disappearance (in units of molarity per second) of A from 100. seconds to 150. seconds? 100 150 250 300 0.00 50.0 200. Time (s) 0.434 0.742 0.254 0.149 0.0870 0.0510 0.0300 [A] (M) Type in the average rate of disappearance as a positive number. Your answer should have three significant figures.
Possible Lewis structures for 6 molecules are shown below. Which figures show correct structures? Correct C:...
Possible Lewis structures for 6 molecules are shown below. Which figures show correct structures? Correct C: Correct » -- :0: Incorrect » :#-$i-: Incorrect - H-j=c-j-HI :o: Incorrect » H-c-5-11 H Correct :C-S-s-c: Check the numbers of valence electrons - all 6 should be neutral molecules, not ions. Submit Answer Incorrect. Tries 1/10 Previous Tries
The experimental data for a Zero order chemical reaction at 25°C is plotted graphically with the...
The experimental data for a Zero order chemical reaction at 25°C is plotted graphically with the resulting linear equation: [C] = 100 - 2t. Where t is in minutes and concentration[C] is in mg/L 1. Determine how long is needed to achieve 95% degradation 2. Determine the half life of the reaction in minutes. 3. If O is 1.2 what is the kinetic constant at 35°C 4. Determine the half life at 35°C.
Consider the reaction at 25°C: 2A (aq) + B (aq) → C (aq) +2D (aq) An...
Consider the reaction at 25°C: 2A (aq) + B (aq) → C (aq) +2D (aq) An experiment was performed with the following initial concentrations: [A] = 2.00 M, [B] = 3.00 M, [C] = 0.100 M, [D] = 0.800 M. The reaction was allowed to proceed until equilibrium was reached at which time [A] = 0.600 M. What is the value of Wmax for the maximum work that could have been performed as the reaction began? Please report your answer...
At a certain temperature, the half-life of the first order decomposition of 2,4-cyclohexadienone (shown below) is...
At a certain temperature, the half-life of the first order decomposition of 2,4-cyclohexadienone (shown below) is 2.11 hr 2,4-cyclohexadienone phenol Answer the following questions about the decomposition of 2,4-cyclohexadienone and report all answers to three significant figures. 1. If the initial concentration of 2,4-cyclohexadienone is 8.04×10-2 M, calculate the time (in hr) required for the concentration of 2,4-cyclohexadienone to decrease to 38.4 % of the initial concentration. Submit Answer Tries o/s 2. If the initial concentration of 2,4-cyclohexadienone is 8.04×10-2...
The velocity v(t) of a sprinter on a straight track is shown in the graph below....
The velocity v(t) of a sprinter on a straight track is shown in the graph below. 11 7 5 v(t) 1 -1 2 10 Determine the evaluaton of each definite integral. Sov(t)dt = 26 S4? (t)dt = 10 5 710 v(t) dt = 4 Soto v(t) dt = 40 Submit Answer Incorrect. Tries 5/8 Previous Tries If s'(t)=v(t), then s(t) is the position of the runner at time t. Let s(0)=-7, determine the following values. s(4) - 13 (5) -...
Most of the time, the rate of a reaction depends on the concentration of the reactant....
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...
Initial rate data are listed in the table for the reaction NH4t (aq)NO2 (aq)N2 (g)H20 () Experiment [NH4+[NO2Initial ra...
Initial rate data are listed in the table for the reaction NH4t (aq)NO2 (aq)N2 (g)H20 () Experiment [NH4+[NO2Initial rate (M/s) 0.10 0.24 7.2 x 104 1 0.10 0.12 3.6 x 104 0.12 0.15 5.4 x 104 0.12 0.12 4.3 x 104 4 First determine the rate law and rate constant Under the same initial conditions as in Experiment 4, calculate [NH4 ] at 368 seconds after the start of the reaction. In this experiment, both reactants are present at the...
Find the rate constant and the initial concentration
I know it's second order, just have no clue how to find K from
this data, or what the initial concentration is. It also says that
the reaction is A -> C
has been studied at 25°C Shown below are the experimental data time (s) [A] (M 1.03 0.811 6 0.669 8 0.569 0.495 10 These data are plotted three different ways, below, as [A] vs t, In[A] vs t and 1/[A]...
At a certain temperature, the half-life of the first order decomposition of phenol (shown below) is 1.54 hr phenol cyclopentadiene carbon monoxide Answer the following questions about the decornposition of phenol and report all answers to three significant figures. 1. If the initial concentration of phenol is 8.73×10 2 M, calculate the time in hr required for the concentration o phenol to decrease to 50.3 % of the initial concentration. Submit Answer Tries 0/3 2. Tf the initial concentration of...
Calculate Reaction Rates From Experimental Data Question Given the data below of the concentration of compound A for the reaction A > B, what is the average rate of disappearance (in units of molarity per second) of A from 100. seconds to 150. seconds? 100 150 250 300 0.00 50.0 200. Time (s) 0.434 0.742 0.254 0.149 0.0870 0.0510 0.0300 [A] (M) Type in the average rate of disappearance as a positive number. Your answer should have three significant figures.
Possible Lewis structures for 6 molecules are shown below. Which figures show correct structures? Correct C: Correct » -- :0: Incorrect » :#-$i-: Incorrect - H-j=c-j-HI :o: Incorrect » H-c-5-11 H Correct :C-S-s-c: Check the numbers of valence electrons - all 6 should be neutral molecules, not ions. Submit Answer Incorrect. Tries 1/10 Previous Tries
The experimental data for a Zero order chemical reaction at 25°C is plotted graphically with the resulting linear equation: [C] = 100 - 2t. Where t is in minutes and concentration[C] is in mg/L 1. Determine how long is needed to achieve 95% degradation 2. Determine the half life of the reaction in minutes. 3. If O is 1.2 what is the kinetic constant at 35°C 4. Determine the half life at 35°C.
Consider the reaction at 25°C: 2A (aq) + B (aq) → C (aq) +2D (aq) An experiment was performed with the following initial concentrations: [A] = 2.00 M, [B] = 3.00 M, [C] = 0.100 M, [D] = 0.800 M. The reaction was allowed to proceed until equilibrium was reached at which time [A] = 0.600 M. What is the value of Wmax for the maximum work that could have been performed as the reaction began? Please report your answer...
At a certain temperature, the half-life of the first order decomposition of 2,4-cyclohexadienone (shown below) is 2.11 hr 2,4-cyclohexadienone phenol Answer the following questions about the decomposition of 2,4-cyclohexadienone and report all answers to three significant figures. 1. If the initial concentration of 2,4-cyclohexadienone is 8.04×10-2 M, calculate the time (in hr) required for the concentration of 2,4-cyclohexadienone to decrease to 38.4 % of the initial concentration. Submit Answer Tries o/s 2. If the initial concentration of 2,4-cyclohexadienone is 8.04×10-2...
The velocity v(t) of a sprinter on a straight track is shown in the graph below. 11 7 5 v(t) 1 -1 2 10 Determine the evaluaton of each definite integral. Sov(t)dt = 26 S4? (t)dt = 10 5 710 v(t) dt = 4 Soto v(t) dt = 40 Submit Answer Incorrect. Tries 5/8 Previous Tries If s'(t)=v(t), then s(t) is the position of the runner at time t. Let s(0)=-7, determine the following values. s(4) - 13 (5) -...
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...
Initial rate data are listed in the table for the reaction NH4t (aq)NO2 (aq)N2 (g)H20 () Experiment [NH4+[NO2Initial rate (M/s) 0.10 0.24 7.2 x 104 1 0.10 0.12 3.6 x 104 0.12 0.15 5.4 x 104 0.12 0.12 4.3 x 104 4 First determine the rate law and rate constant Under the same initial conditions as in Experiment 4, calculate [NH4 ] at 368 seconds after the start of the reaction. In this experiment, both reactants are present at the...
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