![24. The reactants A and B are mixed, and the reaction is timed until a color change occurs. The data are as follows: IA [B] T](http://img.homeworklib.com/questions/90c84890-efe9-11ea-818e-b5c0d1947ea8.png?x-oss-process=image/resize,w_560)
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24. The reactants A and B are mixed, and the reaction is timed until a color...
i just need the answer please, you dont need to go into detail. QUESTION 8 The...
i just need the answer please, you dont need to go into
detail.
QUESTION 8 The reactants A and B are mixed, and the reaction is timed until a color change occurs. The data are as follows: [A] 0.099 0.051 0.101 [B] 0.142 0.143 0.068 Time (s) 104.8 54.0 25.1 The order of the reaction with respect to reactant B is:
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between Aand B, aA+bB⇌cC+dD The dependence of the reaction...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between A and B, aA+bB⇌cC+dD The dependence of the...
Question 23 3 pts Reaction rates at various initial concentrations of reactants were measured at 900°C...
Question 23 3 pts Reaction rates at various initial concentrations of reactants were measured at 900°C for the following reaction 2NO(g) + 2H2(N) + 2 H2O() Use the data in the table to determine the rate law for the reaction. Initial Rate (M/S) Initial [NO] 0.300 0.150 0.250 Initial [H.] 0.100 0.100 0.200 5.69 x 10-2 1.42 x 10- 7.90 x 10- o Rate - k[NO] Hal o Rate - KINOJH2] o Rate -KINO Hal o Rate =kINO] [Hala Question...
Given the equilibrium reaction for a general reaction, A+B <->C, explain what happens to the reactants...
Given the equilibrium reaction for a general reaction, A+B <->C, explain what happens to the reactants and products from time until the time at which the A reaction reaches equilibrium. (Choose any that are correct) Concentration (mol.dm-3) B С Time (s) Once products are formed in a reversible reaction, reactans can not be formed At equilibrium both the reactant and product concentration are the same At time 0, there are no products. At equilibrium all concentrations become constant As the...
B. A scientist had mixed both reactants and products together in a reaction vessel. After some...
B. A scientist had mixed both reactants and products together in a reaction vessel. After some time, thinking the reaction had reached equilibrium, she found that there was 16.6 atm gaseous H2 and 40.0 atm gaseous H2O along with 4.55 g Fe and 3.62 g Fe:04. Had the reaction reached equilibrium? If not, in which direction would the reaction have proceeded to reach equilibrium? EXPLAIN 3. For the given reaction Kp = 0.313: 3Fe(s) + 4H2O(g) =Fe304(s) + 4H2(g) A....
3. A reaction has two reactants A and B. What is the order with respect to...
3. A reaction has two reactants A and B. What is the order with respect to each reactant and the overall order of the reaction described by each of the following rate expressions? a) rate = ki[A] b) rate = k2[A][B] A=3 A=1 B=0 B=1 c) rate = k3[A][B] d) rate = ka[B] A=0 B=a B=1 What are the units of the rate constants in Question 3 if the rate is expressed in mol/L*min? a) b) 4. b)
A certain reaction, A + B → C is first order with respect to each reactant
A certain reaction, A + B → C is first order with respect to each reactant, with k = 1.0 × 10-2 L·mol-1.s-1. Calculate the concentration of A remaining after 100 s if the initial concentration of each reactant was 0.100 M.
C. Given the following data for the reaction A+B products and assuming that the order of...
C. Given the following data for the reaction A+B products and assuming that the order of each reactant does not change with an increase in temperature, answer the following questions. B] 0.100 MO rate (moL-hr) 0.0375 0.0375 0.0750 0.1120 Expt. Temp 2 3 4 25°C 0.100 M 25 C 25°C 45°C 0.100 M 0.200 M 0.100 M 0.500 M 0.100 M 0.200 M 1. How long will it take to use up half of A? 2. At what concentrations of...
Part A The rate of the reaction in terms of the "disappearance of reactant" includes the...
Part A The rate of the reaction in terms of the "disappearance of reactant" includes the change in the concentration of the reactant, the time interval, and the coefficient of the reactant Consider the following reaction: 2A + 3B 3C + 2D The concentrations of reactant A at three different time intervals are given. Use the following data to determine the average rate of reaction in terms of the disappearance of reactant A between time=0s and time = 20 S....
i just need the answer please, you dont need to go into
detail.
QUESTION 8 The reactants A and B are mixed, and the reaction is timed until a color change occurs. The data are as follows: [A] 0.099 0.051 0.101 [B] 0.142 0.143 0.068 Time (s) 104.8 54.0 25.1 The order of the reaction with respect to reactant B is:
Question 23 3 pts Reaction rates at various initial concentrations of reactants were measured at 900°C for the following reaction 2NO(g) + 2H2(N) + 2 H2O() Use the data in the table to determine the rate law for the reaction. Initial Rate (M/S) Initial [NO] 0.300 0.150 0.250 Initial [H.] 0.100 0.100 0.200 5.69 x 10-2 1.42 x 10- 7.90 x 10- o Rate - k[NO] Hal o Rate - KINOJH2] o Rate -KINO Hal o Rate =kINO] [Hala Question...
Given the equilibrium reaction for a general reaction, A+B <->C, explain what happens to the reactants and products from time until the time at which the A reaction reaches equilibrium. (Choose any that are correct) Concentration (mol.dm-3) B С Time (s) Once products are formed in a reversible reaction, reactans can not be formed At equilibrium both the reactant and product concentration are the same At time 0, there are no products. At equilibrium all concentrations become constant As the...
B. A scientist had mixed both reactants and products together in a reaction vessel. After some time, thinking the reaction had reached equilibrium, she found that there was 16.6 atm gaseous H2 and 40.0 atm gaseous H2O along with 4.55 g Fe and 3.62 g Fe:04. Had the reaction reached equilibrium? If not, in which direction would the reaction have proceeded to reach equilibrium? EXPLAIN 3. For the given reaction Kp = 0.313: 3Fe(s) + 4H2O(g) =Fe304(s) + 4H2(g) A....
3. A reaction has two reactants A and B. What is the order with respect to each reactant and the overall order of the reaction described by each of the following rate expressions? a) rate = ki[A] b) rate = k2[A][B] A=3 A=1 B=0 B=1 c) rate = k3[A][B] d) rate = ka[B] A=0 B=a B=1 What are the units of the rate constants in Question 3 if the rate is expressed in mol/L*min? a) b) 4. b)
C. Given the following data for the reaction A+B products and assuming that the order of each reactant does not change with an increase in temperature, answer the following questions. B] 0.100 MO rate (moL-hr) 0.0375 0.0375 0.0750 0.1120 Expt. Temp 2 3 4 25°C 0.100 M 25 C 25°C 45°C 0.100 M 0.200 M 0.100 M 0.500 M 0.100 M 0.200 M 1. How long will it take to use up half of A? 2. At what concentrations of...
Part A The rate of the reaction in terms of the "disappearance of reactant" includes the change in the concentration of the reactant, the time interval, and the coefficient of the reactant Consider the following reaction: 2A + 3B 3C + 2D The concentrations of reactant A at three different time intervals are given. Use the following data to determine the average rate of reaction in terms of the disappearance of reactant A between time=0s and time = 20 S....
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