Homework Answers
In this titration, the analyte is oxalic acidand the titrant is potassium permanganet It is a redox reaction. The oxalic acid acts as a reducing agent, and the KMnO4 acts as an oxidizing agent. Since the reaction takes place in an acidic medium, the oxidizing power of the permanganet ion is increased.
Order of reaction with respect to both oxalic acid and potassium permanganet is 1 and the overall reaction order is 2.
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1. Calculate the order of reaction with respect to: a) H2C204 b) KMnO4
For problems #11-13. Use the data below to answer the questions: KMnO4 + H2C204 -----> Products...
For problems #11-13. Use the data below to answer the questions: KMnO4 + H2C204 -----> Products Reaction KMnO4 (M) H2C204 (M) Initial rate (M/s) 1) 0.02167 0.2517 5.599 x 10-5 2) 0.04330 0.2517 1.312 x 10-4 3) 0.02167 0.5030 9.029 x 10-5 Using the reaction equation above, choose the rate law that describes this reaction Rate = K[KMnO4)² [H2C204] Rate = K[KMnO4)2 [H2C2041 K[KMnO4][H2C20412 Rate = Rate = K[KMnO4) (H2C2041 None of these describes the actual reaction's rate.
A reaction is second order with respect to [A] and half order with respect to [B]....
A reaction is second order with respect to [A] and half order with respect to [B]. A. Write the rate law for this reaction. B. If [A] increases by a factor of 9, while [B] remains constant, by what factor will the Rate of reaction change
8. For the reaction r = k [I2] ^ 2 [KMnO4] ^ 3 we can establish...
8. For the reaction r = k [I2] ^ 2 [KMnO4] ^ 3 we can establish that: a.the reaction is second order with respect to iodine b. the reaction is fifth order c. the reaction is third order with respect to KMnO4 d. all of the above
1. The reaction A → B + C is zero order with respect to A. When...
1. The reaction A → B + C is zero order with respect to A. When [A]0 = 0.544 M, the reaction is 28 % complete at 91.5 min. Calculate the half-life for this reaction. 2. Consider the following reaction. Calculate the value of the rate constant.. 2 A + B →→ 2 C A B C Rate Trial 1 0.64 0.56 0.012 7.463 Trial 2 1.28 0.56 0.012 14.926 Trial 3 0.64 1.12 0.012 14.926 Trial 4 0.1...
The reaction The reactionA -> B+C is second order with respect to A. When [A]0= 0.290...
The reaction The reactionA -> B+C is second order with
respect to A. When [A]0= 0.290 M the reaction is 43.0% complete at
64.5 min. calculate the half life for this reaction.
The reaction A B+C is second order with respect to A. When [Alo 0.290 M, the reaction is 43.0 % complete at 64.5 min. Calculate the half-life for this reaction.
The following reaction is second order in respect to NO and first order in respect to...
The following reaction is second order in respect to NO and first order in respect to H2. The rate constant was found to be 0.67 M-2· s-1. If the reaction starts with 0.200 M NO and 0.350 M H2, calculate the initial reaction rate. Group of answer choices 0.0094 M/s 0.047 M/s 0.014 M/s 0.0022 M/s
The reaction A+B → products is of the first order with respect to the reagent A...
The reaction A+B → products is of the first order with respect to the reagent A and second order with respect to reagent B. A.) Write the speed law for reaction B.) What is the value of the constant of speed of the reaction C.) Complete the table Experiment 1 (B) 0.200 M 1 IWNL (A) .00 M 2.00 M 2.00 M Velocity (m/s) 0.150 0.300 0.400 M
You have a reaction: A + B --> C The reaction is first order with respect...
You have a reaction: A + B --> C The reaction is first order with respect to A and 2nd order with respect to B. If 0.8904 mol of A is mixed with 0.3749 mol of B to make a 1.000 L solution and the rate of the reaction is 0.873 M/s, what is the rate constant (k)?
The reaction 2A + 3B → C is first order with respect to A and B....
The reaction 2A + 3B → C is first order with respect to A and B. When the initial concentrations are [A] 1.55 x 10 2 M and [B] 2.11 × 10-3 M, the rate is 2.65 x 10 4 M. Calculate the rate constant or the reaction. Enter your answer in scientific notation. 10 O M ● M-1 M1.s1
The reaction A+B → products is of the first order with respect to the reagent A...
The reaction A+B → products is of the first order with respect to the reagent A and second order with respect to reagent B. A.) Write the speed law for reaction B.) What is the value of the constant of speed of the reaction C.) Complete the table Experiment (A) 1.00 M 2.00 M 2.00 M 0.200 M Velocity (m/s) 0.150 0.300 0.400 M
For problems #11-13. Use the data below to answer the questions: KMnO4 + H2C204 -----> Products Reaction KMnO4 (M) H2C204 (M) Initial rate (M/s) 1) 0.02167 0.2517 5.599 x 10-5 2) 0.04330 0.2517 1.312 x 10-4 3) 0.02167 0.5030 9.029 x 10-5 Using the reaction equation above, choose the rate law that describes this reaction Rate = K[KMnO4)² [H2C204] Rate = K[KMnO4)2 [H2C2041 K[KMnO4][H2C20412 Rate = Rate = K[KMnO4) (H2C2041 None of these describes the actual reaction's rate.
The reaction The reactionA -> B+C is second order with
respect to A. When [A]0= 0.290 M the reaction is 43.0% complete at
64.5 min. calculate the half life for this reaction.
The reaction A B+C is second order with respect to A. When [Alo 0.290 M, the reaction is 43.0 % complete at 64.5 min. Calculate the half-life for this reaction.
The reaction A+B → products is of the first order with respect to the reagent A and second order with respect to reagent B. A.) Write the speed law for reaction B.) What is the value of the constant of speed of the reaction C.) Complete the table Experiment 1 (B) 0.200 M 1 IWNL (A) .00 M 2.00 M 2.00 M Velocity (m/s) 0.150 0.300 0.400 M
The reaction 2A + 3B → C is first order with respect to A and B. When the initial concentrations are [A] 1.55 x 10 2 M and [B] 2.11 × 10-3 M, the rate is 2.65 x 10 4 M. Calculate the rate constant or the reaction. Enter your answer in scientific notation. 10 O M ● M-1 M1.s1
The reaction A+B → products is of the first order with respect to the reagent A and second order with respect to reagent B. A.) Write the speed law for reaction B.) What is the value of the constant of speed of the reaction C.) Complete the table Experiment (A) 1.00 M 2.00 M 2.00 M 0.200 M Velocity (m/s) 0.150 0.300 0.400 M
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