Q: What Are the Mechanisms of Catalysis?
A: For every chemical reaction there is a rate at which the reaction proceeds. Some reaction occur…
Q: Account for the relationship between the rate of a reaction and its activation energy.
A: Concept introduction: Activation energy of a reaction is the minimum amount of energy that is to be…
Q: units for the rate constant,
A: This is a 2nd order reaction . unit of K = (mol/(L.min)) / (mol/L)2 = mol -1 . L…
Q: What is the rate law for the reaction?
A: Answer The rate law A rate law is an expression for the the relationship of…
Q: Define the rate of the reaction HBr in the following reaction
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Q: In what type of reaction would the instantaneous rate stay constant throughout the reaction?
A: The instantaneous rate is the rate of a reaction at any specific time. The reaction for which the…
Q: The rate constant for a reaction can be increased by ______ the stability of the reactant or by…
A:
Q: Consider the data on "Initial Rates" Provided in the table, for the following reaction.
A: To solve this problem we have consider the experimental data given in table . From this data we will…
Q: The magnitude of the rate constant for the reaction is:
A:
Q: Give the rate equation describing the reaction. How long will the reaction take to come to an end.…
A: According to the previous calculations, the reaction is 1st order with respect to the reactant…
Q: What is rate law?
A: The mathematical relationship of reaction rate with reactant concentrations is known as the rate…
Q: Does the rate constant for a reaction generally increase or decrease with an increase in reaction…
A: Kinetics of reaction tells about the rate of reaction. Reaction rate decrease or increase depending…
Q: What are the implications for the reaction rate of a negative Reaction Order?
A: Order of reaction can be negative or positive.
Q: What role does adsorption play in the action of a heterogeneous catalyst?
A: The role of adsorption in the action of a heterogeneous catalyst is given as,
Q: how to use a table to figure out the rate constant
A: Firstly we will have a equation, reaction between nitrogen monoxide and hydrogen gas to form…
Q: Define Heterogeneous Catalysis?
A: Heterogeneous Catalysis can be defined as a type of catalysis where catalyst is in different phase…
Q: 2. The rate constant for the forward reaction is equal to the rate constant of the reverse reaction.
A: At equilibrium concentrations of reactants and products remain unchanged. In other words the…
Q: How do the rate of a reaction and its rate constant differ?
A: Chemical kinetics gives the study of the rate of reaction at which it can occur.
Q: explain why the rate of reaction initially increases with temp?
A: The objective of the question is to explain the reason of increase of rate of reaction initially…
Q: a) Express the rate of the reaction in terms of the change in concentration of each of the reactants…
A: Rate = -1/2 ∆[H2]/dt =-(0.067-1.00)/(40-0)*2 =0.0116625
Q: When a reaction is cooled, what effect will this have on the rate of reaction and why?
A: It has been observed that the rate constant for a chemical reaction gets doubled for every 10oC rise…
Q: 4. What is a reaction mechanism?
A: Since you have posted multiple questions as per guidelines we can answer only one per session . If…
Q: Obtain the rate law based on the kinetic study of the reaction.
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Q: Define the molecularity of a reaction and explain how and when this is linked to the reaction…
A: Molecularity: The molecularity of a reaction is described as the number of reacting molecules that…
Q: What information can be extracted from the determination of the rate of a chemical reaction under…
A: Information can be extracted from the determination of the rate of a chemical reaction under…
Q: Why is it important to know the reaction rates? What are the factors affecting rate of reaction? Why…
A: Rate of reaction is that speed of reaction at which a chemical reaction is taking place in a system.…
Q: What is the rate law for this reaction?
A: Given reaction is A+ 2B ↔C Let the general rate law of given reaction is Rate = k[A]x [B]y where…
Q: What is half-life period of a reaction?
A: A reaction consists of reactants and there is the formation of products.
Q: Determine the reaction order, the rate constant, and the units of the rate constant.
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Q: The units of the rate constant depend on the order of the reaction.
A: A + B -------> products According to the rate law :- Rate = k[A]a[B]b Where k is the rate…
Q: the rate constant k for a first order reaction is what?
A: Rate Constant k for a First order reaction: Consider the reaction,
Q: Given the image, what is the rate law of the reaction.
A: Let the rate law of the reaction be: Rate=k[NO2]a[O3]b ...... (1) Putting the…
Q: How can we determine the rate constant for the reaction?
A: Rate constant tells about the rate of the reaction. Higher the rate constant higher is the rate of…
Q: Under what three conditions are reactions said to be irreversible?
A: The reaction in which the entire amount of reactants is converted into the product is called…
Q: Can you propose a way by which the rate of reaction may be quantitatively measured?
A: Rate of Reaction- The rate of a reaction is usually observed by watching the disappearance of a…
Q: What part of the rate law is temperature dependent?
A: The increase in the rate of reaction with rise in temperature is not due to the increase in the…
Q: calculate the rate constant of the reaction. O
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Q: Calculate the average rate constant for the reaction.
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Q: What is meant by the rate of a chemical reaction? What are the units of the rate of a reaction?
A: Hi, since you have posted multiple questions. We will answer the very first question. Kindly repost…
Q: does a caralyst change the rate constant of a reaction?
A: Catalyst is a biological enzyme which increases the rate of reaction by decreasing the activation…
Q: Define the term Average Rate of Reaction?
A: Rate of a chemical reaction is defined as the speed with which the reaction proceeds. It determines…
Q: Does the rate constant depend on the concentrations of the reactants?
A: Rate constant:- It is defined as the rate of reaction when the concentration of reactants taken as…
Q: the rate constant for the reaction is
A:
Q: What is the reaction constant and the rate law of the reaction in the table?
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Q: What is the difference between reaction rate and the specific rate constant (k)?
A: Given : Reaction rate and specific rate constant i.e k.
Q: Write two differences between ‘order of reaction’ and ‘molecularity of reaction’.
A: Reaction order: It refers to the power dependence of the rate on the concentration of each reactant.…
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- centropy (randomness) 10. Arrange the following reactions in order of increasing AS value. 1. H₂(g) + F2(g) → 2HF(g) зд 2. NH4NO3(s) → N₂O(g) + 2H₂O() 19, 12, 15 3. (NH4)2Cr2O7(s) →→→ Cr2O3(s) + 4H₂O(l) + N₂(g) 1,1g, 25The following data was collected for the reaction between ethoxide and methyl iodide T(°C) Rate (1/s) T (K) 1/T (1/K) In (rate) 168 273.15 0.00366 5.12 6 354 279.15 0.00358 5.87 12 735 285.15 0.00351 6.60 18 1463 291.15 0.00343 7.29 24 3010 297.15 0.00337 8.01 30 6250 303.15 0.00330 8.74 A plot of In (rate) vs. 1/T using the above table was made and is shown below, and a linear regression line fitted to the data. Using the provided graph, estimate the activation energy (kJ/mol) of the reaction between ethoxide and methyl iodide. Enter your number using 2 decimal places without unit. Gas constant is R = 8.3144598 J. mol 1. K-1. In(k) vs 1/T 9.30 8.80 8.30 7.80 y = -9930.5x + 41.445 R² = 0.9992 2 7.30 6.80 6.30 5.80 5.30 4.80 0.00325 0.00330 0.00335 0.00340 0.00345 0.00350 0.00355 0.00360 0.00365 0.00370 1/T (1/K) Ln(k)2. Consider the kinetic data of the reaction of P + 2 Q + 2+ - PQ, + Z*and answer the succeeding questions: Experiment P (M) Q (M) Temp ("C) Initial Rate, M/s 1 0.01150 0.01200 0.00000 25 4.80 x 10-4 2 0.02300 0.01200 0.00000 25 1.92 x 10-3 3 0.01150 0.02400 0.00000 25 9.60 x 10-4 4 0.04600 0.01200 0.00000 25 7.68 x 10-3 5 0.01150 0.04800 0.00000 25 1.92 x 10-3 6 0.01150 0.01200 0.00000 10 5.10 x 10-5 0.01150 0.01200 0.00000 40 4.55 x 10-3 0.01150 0.01200 0.00500 10 4.98 x 10-5 0.01150 0.01200 0.01050 25 4.82 x 104 10 0.01150 0.01200 0.02100 40 4.44 x 10-3 A. Determine the rate order with respect to P. Determine the rate order with respect to Q. C. Determine the rate law of the reaction. What is the average rate constant? Indicate the appropriate units. E. What is the energy of activation and frequency factor of the reaction without the additive ion? Include the equation of the best fit line of the Arrhenius equation and RSQ Note: Use the calculated rate constant in set up 1 for 25°C…
- 3. The reaction H₂SO3(aq) + 6(aq) + Haq) → Se(s) +213(aq) + 3H₂0 (1) was studied at 0°C. The following data were obtained: Experiment # 1 2 3 4 5 6 7 [H₂SO3(aq)lo (mol/L) constant? 1.0 x 104 2.0 x 10-4 3.0 x 104 1.0 x 10-4 1.0 x 10-4 1.0 x 104 1.0 x 104 [¹] (mol/L) 2.0 x 10² 2.0 x 10-² 2.0 x 10-² 4.0 x 10-² 1.0 x 10-² 2.0 x 10-² 1.0 x 10-² Find the order of the reaction with respect to [H₂SO3]. respect to [I-¹]. reaction with respect to [H+¹]. is the overall order of the reaction? Find the value of the rate constant (k). Only write the number. [H¹+] (mol/L) 2.0 x 10-² 2.0 x 10-² 2.0 x 10-² 2.0 x 10-² 2.0 x 10-² 4.0 x 10-² 4.0 x 10-² Rate (mol/L.s) Find the order of the reaction with Find the order of the What What are the units of the rate 1.66 x 10-7 3.33 x 10-7 4.99 x 10¹7 6.66 x 10-7 0.42 x 10-7 13.2 x 10-7 3.36 x 10-7DETERMINATION OF A,H FOR THE REACTION OF Mg AND HCl Minimize D The results from one run are shown below. 40 00003333333t1&C66C0000000000333333113ttteeccc000000 y = -0.51215 x + 40.274 20 10 4 5 Time (min) Q3 Use the graph to determine Tinitial and Tfinal. You must then use these values to calculate the change in temperature for the reaction. Tinitial (°C) Tinal (°C) AT (°C) 1 2 Temperature (°C) 30Predicting relative forward and reverse rates of reaction in a... Acetic acid and ethanol react to form ethyl acetate and water, like this: HCH,CO,(aq)+c,H,OH(aq) → C,H,CO,CH;(aq)+H,0(1) Imagine 137. mmol of c,H,CO,CH, are removed from a flask containing a mixture of HCH3CO,, C2H¿OH, C,H,CO,CH; and H,0 at equilibrium, and then answer the following questions. O Zero. What is the rate of the reverse reaction before any C2H5CO2CH3 has been removed from the flask? O Greater than zero, but less than the rate of the forward reaction. Greater than zero, and equal to the rate of the forward reaction. Greater than zero, and greater than the rate of the forward reaction. O Zero. What is the rate of the reverse Greater than zero, but less than the rate of the forward reaction. reaction just after the C2H5CO2CH3 has been removed from the flask? Greater than zero, and equal to the rate of the forward reaction. Greater than zero, and greater than the rate of the forward reaction. Zero. What is the…
- 10:15 1 Question 7 of 25 Submit Construct the expression Kc for the following reaction. Sn(s) + 4 Cl2(g) =2 SnCl4(1) 1 Drag the tiles into the numerator or denominator to form the expression. K. = 5 RESET [SnCl.] [Cl.] [Sn] 2[SnCl4] 4[Cl2] 2[Sn] [SnCl.]? [Cl,]* [Sn]? 2[SnCl.]? 4[Cl_]* 2[Sn]?11:08 1 Question 23 of 25 Submit Construct the expression Kc for the following reaction. 2 P(s) + 5 Cl2(g) = 2 PCI;(g) 1 Drag the tiles into the numerator or denominator to form the expression. K. = 5 RESET [P] [Cl.] [PCIg] 2[P] 5[Cl_] 2[PCI;] [P]? [PCIs]? 2[P]? 5[Cl_]$ 2[PCIs]?5. Target Reaction: 20 H O(1) + 2H 0) 2C H O) + O_() 2 4 Step Reactions: 2 C2H601) + 302(g) → 2CO2(g) + 3H2OO C2H40(1) + 5/202(g) → 2CO2(g) + 2H2O(1) AH = -685 kJ AH = -583.5 k-
- Ne(g) effuses at a rate that is ______ times that of Kr(g) under the same conditions. rateNe/rateKr=Years and the table of standard formation and thaws but your fine under the alexs dedicate tabs calculate the reaction empathy of the reaction under standard conditions 2HNO2g+O2g=2HNO3gB' B D' E Es (E in kJ) Reaction progress → Match the labels with the correct quantities by examining the diagram above: E, + Ez 1. Ealfwd), uncatalyzed 2. Ea(rev), uncatalyzed 3. enthalpy change, forward reaction B 4. activated complex, uncatalyzed E1 reaction A 5. reactants Eg - Eg 6. enthalpy change, reverse reaction 7. activated complex, catalyzed D reaction Eg - E4 8. products Energy of onolecules > D000