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Areaction was found to be zero-order in A and third-order in B. Increasing the concentration of...
A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction...
A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to? increase by a factor of 27 increase by a factor of 9 triple decrease by a factor of the cube root of 3
The reaction A+B → products was found to have the rate law; rate = k[A][B]2. While...
The reaction A+B → products was found to have the rate law; rate = k[A][B]2. While holding the concentration of B constant, the concentration of A was increased from 0.010M to 0.030M. Predict by what factor the rate of reaction will increase. Select one: a. 9 b.3 c. No effect d. 16 e. 6
Part A) The reactant concentration in a zero-order reaction was 7.00×10−2 M after 200 s and...
Part A) The reactant concentration in a zero-order reaction was 7.00×10−2 M after 200 s and 1.50×10−2 M after 370 s . What is the rate constant for this reaction? Part C) The reactant concentration in a first-order reaction was 7.90×10−2 M after 45.0 s and 2.00×10−3 M after 75.0 s . What is the rate constant for this reaction? Part D) The reactant concentration in a second-order reaction was 0.690 M after 220 s and 5.00×10−2 M after 825...
1. A reaction is second order in[A] and second-order in [B]: Rate,=K[A]^2[B]^2. what are the units...
1. A reaction is second order in[A] and second-order in [B]: Rate,=K[A]^2[B]^2. what are the units of k for this reaction? If the concentration of air decreases by a factor of 2 and the concentration of b increases by a factor of 5 what happens to the rate? 2. for the forward reaction 2NO+Cl2=>2NOCl. determine the rate(m/s)for experiment #4 given [NO]°(M)=0.40M and [Cl2]°z(M)=0?20M. Rate? 3.The following data were collected over time for the forward reaction 2NO2=>2NO+O2 ( 1/[NO2]=100 at 0...
A reaction in which A, B, and C react to form products is zero order in...
A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. Part A Write a rate law for the reaction. O Rate = k [A] [B] [C]1/2 O Rate = k [B] [C]1/2 Rate = k [B]1/2 [C] Rate = k [A] [B]1/2 [C] Submit Request Answer Part B What is the overall order of the reaction? Express your answer numerically. EVO AEQ O 2...
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration...
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration of NOBr was followed as a function of time. It was found that a graph of 1/[NOBr] versus time in seconds gave a straight line with a slope of 1.27 m?s and a y-intercept of 3.98 M? Based on this plot, the reaction is order in NOBr and the rate constant for the reaction is M?? In a study of the decomposition of hydrogen...
The reaction A B + 2 C is known to be zero order in A and to have...
The reaction A B + 2 C is known to be zero order in A and to have a rate constant of 3.0 x 10–1mol/L. An experiment was run at 25°C and initial concentration of reagent [A] = 2.0 x 10–3 M. What is the rate of the reaction? Unable to predict. The rate of the reaction is 3.0 x 10–1 mol/L. The rate of the reaction is 2.0 x 10–3 mol/L. The rate of the reaction is 6.0 x 10–4 mol/L.
The reactions in the table are all zero order and follow the same general reaction process...
The reactions in the table are all zero order and follow the same general reaction process of A → products. Half-life, 112 (8) Rate constant, * (M.5-) Initial concentration, [A]. (M) Reaction 1 3.71 0.0731 ? Reaction 2 0.0671 0.971 Reaction 3 5.11 ? 0.411 Reaction 4 4.31 0.0771 ? Reaction 5 4.31 0.371 ? ? Calculate the missing values for half-life (fin), rate constant (k), and initial concentration, (Alo. reaction 1 initial concentration, (Alo: M action 2 half-life, 112...
A reaction is found to be 0th order with respect to thiosulfate ion. If the concentration...
A reaction is found to be 0th order with respect to thiosulfate ion. If the concentration of thiosulfate ion is 0.159M after 20.5 seconds have passed, and the rate law constant is 0.0175 M/sec, what was the initial concentration of thiosulfate ion?
A reaction is found to be 2nd order with respect to cyanide ion. If the concentration...
A reaction is found to be 2nd order with respect to cyanide ion. If the concentration of cyanide ion is 0.175M after 16.9 seconds have passed, and the rate law constant is 0.0201 M/sec, what was the initial concentration of cyanide ion?
A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to? increase by a factor of 27 increase by a factor of 9 triple decrease by a factor of the cube root of 3
The reaction A+B → products was found to have the rate law; rate = k[A][B]2. While holding the concentration of B constant, the concentration of A was increased from 0.010M to 0.030M. Predict by what factor the rate of reaction will increase. Select one: a. 9 b.3 c. No effect d. 16 e. 6
A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. Part A Write a rate law for the reaction. O Rate = k [A] [B] [C]1/2 O Rate = k [B] [C]1/2 Rate = k [B]1/2 [C] Rate = k [A] [B]1/2 [C] Submit Request Answer Part B What is the overall order of the reaction? Express your answer numerically. EVO AEQ O 2...
In a study of the decomposition of nitrosyl bromide at 10 °C NOBr—+NO+ Br2 the concentration of NOBr was followed as a function of time. It was found that a graph of 1/[NOBr] versus time in seconds gave a straight line with a slope of 1.27 m?s and a y-intercept of 3.98 M? Based on this plot, the reaction is order in NOBr and the rate constant for the reaction is M?? In a study of the decomposition of hydrogen...
The reactions in the table are all zero order and follow the same general reaction process of A → products. Half-life, 112 (8) Rate constant, * (M.5-) Initial concentration, [A]. (M) Reaction 1 3.71 0.0731 ? Reaction 2 0.0671 0.971 Reaction 3 5.11 ? 0.411 Reaction 4 4.31 0.0771 ? Reaction 5 4.31 0.371 ? ? Calculate the missing values for half-life (fin), rate constant (k), and initial concentration, (Alo. reaction 1 initial concentration, (Alo: M action 2 half-life, 112...
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