# Rate Law

### Topic Page

Rate Law### Questions

- How do catalysts affect rates of reaction?
- How do enzymes speed up rates of reaction?
- How do rates of reaction change with concentration?
- How does temperature affect the rate of reaction?
- How are reaction rate and equilibrium related?
- What influences reaction rates?
- Is the reaction rate affected by surface area?
- Does volume affect the reaction rate?
- How does pressure affect the reaction rate?
- How do you find rate law for a reaction?
- How do you calculate the average rate of a reaction?
- How does the reaction rate change with time?
- How do enzymes increase reaction rates?
- How do coefficients affect the rate law?
- What is an integrated rate law?
- How is the reaction rate related to equilibrium?
- Does the rate law change with temperature?
- What is a reaction rate?
- What are some common mistakes students make with rate law?
- What are some examples of rate law?
- Question #9c0e4
- Question #44fac
- Question #e6a1f
- Question #5b733
- A viral preparation was inactive in a chemical broth. The inactivation process was found to be 1st order in viral concentration. At the beginning of the experiment 2.0% of virus was found to be inactive/min. Evaluate the k for the inactivation process?
- 2 NOBr (g) - 2NO (g) + Br2 (g) Given the rate is -2.3 mol NOBr L-1hr-1 when the initial concentration was 6.2 M what is the rate constant k? Assume the reaction is 1st order in [NOBr]
- The first order rate constant for hydrolysis of CH3Cl in H2O has a value of 3.32x10-10 s-1 at 25oC and 3.13x10-9 s-1 at 40oC. What is the activation energy?
- Question #50095
- Question #3a8f6
- Question #8a56f
- Question #26863
- Question #91357
- Question #161ec
- Question #a6130
- The data below were collected for the following reaction at a certain temperature: #X_2Y→2X+Y# (Data found as picture in answer box). What is the concentration of #X# after 12 hours?
- Question #b354b
- Question #a5353
- Question #7d5f5
- The reaction #"A + 2B → C +D"# is first-order in the concentrations of **A** and **B**. What is the concentration of **C** after 10 s if the initial concentrations of **A** and **B** are 0.025 mol/L and 0.150 mol/L, respectively?
- Question #c81c4
- Question #a6570
- Question #47c93
- Question #c4b96
- Question #5c648
- In a second order reaction, the concentration of #A# has dropped to #"0.020 M"# in one hour. If the initial concentration of #A# is #"0.050 M"# and that of #B# is #"0.080 M"#, what is the rate constant? What then is the half-life, if #[B]# is held fixed?
- Question #14f66
- Question #dd444
- For the following reaction, find the rate law and rate constant? #2"NO"(g) + "O"_2(g) -> 2"NO"_2(g)#
- A first order reaction is 50% completed after 30 minutes.This implies that the time required to complete 90% of the reaction is?
- Could you derive the rate law for two competing first order reactions and the formula for the product ratio, please?
- What is the rate constant of a reaction if rate 1.5 (mol/L)s, [A] is 1 M, [B] is 3 M, m=2, and n=1?
- Question #7f455
- For the reaction #"N"_2"O"_3(g) -> "NO"(g) + "NO"_2(g)#, given the following data, calculate the rate constant?
- Question #a0e43
- Question #9f11e
- How to derive the following formula? [Pressure in relation to kinetics]
- What role do elementary reactions play in determining reaction order with respect to each reactant? How is the mechanism related to how a rate constant for a complex reaction compares to that of a one-step reaction?
- What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: #A + B leftrightarrow C# (fast) Step 2: # B + C -> D# (slow)
- Consider the following reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) Use the data below to find the rate law and determine the value of the rate constant? Make sure to report proper units!
- Write the rate law for this reaction, and give the numerical value of the rate constant?
- Give the form of the rate law for this reaction?
- If the activation energy for a given compound is found to be 42.0 kJ/mol, with a frequency factor of #8.0 x 10^10 s^(-1)#, what is the rate constant for this reaction at 298 K?
- The reaction rate law is known to be 2nd order, and for an initial concentration [NO2(g)]o=0.0100M, the initial rate is 0.0350 M/s. Write the rate law, and give the value of the rate constant?
- A certain reaction follows zero-order kinetics. Suppose the reaction went to #50%# completion after #10# minutes. What percentage of completion does the reaction reach in an additional #5# minutes?
- What is the volume after 5 hours in this first order reaction?
- The reaction #2NO_2 -> 2NO + O_2# obeys the rate law #(Delta[O_2])/(Deltat) = (1.40 xx 10^-2 )[NO_2]^2# at 500 K. If the initial concentration of #NO_2# is 1.00 M, how long will it take for the #[NO_2]# to decrease to 25.0% of its initial value?
- If the initial concentration of #"AB"# in #AB(g) -> A(g) + B(g)# is #"1.50 M"#, and #k = "0.80 M"^(-1)cdot"s"^(-1)#, what amount of time passes until the concentration becomes #1//3# of what it began as in this second-order decomposition?
- Question #45ea5
- Question #f875f
- The data in the tablebe ow were obtained for the reaction: #A + B -> P#. What is the rate law for this reaction?
- The rate law of a reaction is rate = k[D][X]. What are the units of the rate constant?
- #H_2(g) + 2NO(g) -> H_20(g) + N_2O(g)#. At high temperatures, doubling the concentration of #H_2# doubles the rate of reaction, while doubling the concentration of #NO# increases the rate fourfold. How do you write a rate law for this reaction?
- Question #e6605
- Question #fcc15
- For the reaction #2"NO"(g) + "Br"_2(g) -> 2"NOBr"(g)#, the following data were obtained. What is the rate constant?
- What are the orders of #"CV"^(+)# and #"OH"^(-)# for the reaction #"CV"^(+)(aq) + "OH"^(-)(aq) -> "CVOH"(aq)#?
- What are the units of the rate constant, k, for the decomposition of #H_2O_2#(aq)?
- How do you find the integrated rate laws for zeroth, first, and second order reactions?
- Question #cf765
- Question #fa922
- What equation relates concentration to temperature #t#?
- How do I find the order for each reactant?
- How do you find the rate law for the following overall reaction, given its mechanism below? #2A + C -> D#
- Rate law quick question??
- Find the following for the reaction #"NO"(g) + "O"_3(g) -> "NO"_2(g) + "O"_2(g)#?
- Question #59ea6
- The half-life of titanium-44 is 63 years. What is the constant k in the decay formula for the substance?
- Question #10bf9
- The reaction? H2(g)+ I2(g)---> 2HI(g) may occur by the following mechanism: k1(--->) I2<=>2I (fast, equilibrium) k-1(<---) I + I + H2 ---> 2HI (slow) k2
- Find the rate law of #2NO+2H_2\rarrN_2+2H_2O# for the following table below?
- Determine rate law and rate constant for #2"I"^(-)(aq) + "S"_2"O"_8^(2-)(aq) -> "I"_2(aq) + 2"SO"_4^(2-)(aq)#?
- An 80.0 sample of #N_2O_5# is allowed to decompose at 45°C, how long does it take for the quantity of #N_2O_5# to be reduced to 2.5 g?