Rate laws or rate equations are mathematical expressions that describe the relationship between the rate of a chemical reaction and the concentration of its reactants. In general, a rate law (or differential rate law, as it is sometimes called) takes this form:
rate=k[A]m[B]n[C]p
in which [A], [B], and [C] represent the molar concentrations of reactants, and k is the rate constant, which is specific for a particular reaction at a particular temperature.The exponents m, n, and p are usually positive integers (although it is possible for them to be fractions or negative numbers).
for first equation,
2A + B = C + D
rate= k [A]2 [B]
for second equation,
X + Y = Z
rate= k [X] [Y]
Write the rate law for the two elementary reaction equations. 2 A(g) + B(g) → C(g)...
Consider the elementary reaction equations shown. A(g) + B(g) --> C(g) + D(g) 2X(g) --> Y(g) + Z(g) Write the rate law for reaction A. Write the rate law for reaction B.
5. An elementary reaction has the form 2A → B. The rate law is Rate A) k[A] B) 2 k[A] C) k? [A] D) k[A] 6. For some reaction, when concentration of reactant "A" doubles, the rate of the reaction doubles. The reaction is order in reactant A. B) 1" A oth C) 2nd D) 3rd 7. Tetrahydrofuran (commonly referred to as THF) is an organic solvent with a density of 0.889 g/mL. A solution is prepared by dissolving 11.8...
To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. Very often, a reaction does not tell us the whole story. For instance, the reaction NO2(g)+CO(g)→NO(g)+CO2(g)NO2(g)+CO(g)→NO(g)+CO2(g) does not involve a collision between an NO2NO2 molecule and a COCO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: NO2(g)+NO2(g)→NO3(g)+NO(g)NO2(g)+NO2(g)→NO3(g)+NO(g) NO3(g)+CO(g)→CO2(g)+NO2(g)NO3(g)+CO(g)→CO2(g)+NO2(g) Each individual step is called an elementary step. Together, these...
2.c and 2.d 2. The rate law for the reaction A+B a. Write the rate law expression. C + D is first order in [A] and second order in [B]. Rate low- k[A] [B]² b. What is the overall order of reaction? 1 +2= 3 c. How does the rate change if [A] is halved and [B] is tripled?! d. Given the data below, propose initial concentrations for A and B that would enable you to empirically determine the given...
8) A reaction occurs via the following sequence of elementary steps. What is the rate law based on this reaction mechanism? very fast slow fast 1st step: A B 2nd step: B+C D 3rd step: D - 2E A) rate = k[E]2 B) rate = k[A] [C] C) rate = k[B][C] D) rate = k[D] E) rate = k[A] [B]
Substance A and B react in elementary steps according to the following equations: Step 1: A+B --> C+D k=0.25M/min Step 2: D+A --> C+E k=0.0002M/min a) Determine the equation for the overall reaction. b) Give the expected rate law for the reaction from the information above.
For the chemical reaction: A + B 3 C observed to have a rate law of Rate = k [B]2, the following reaction mechanism has been proposed. 2 B D (slow) D + A 3 C + B In your evaluation of the reaction mechanism you would conclude the mechanism is: A) a plausible representation of the reaction B) an implausible representation as the predicted rate law does not match the observed rate law C) an implausible...
1) A certain reaction has an activation energy of 67.68 kJ/mol.67.68 kJ/mol. At what Kelvin temperature will the reaction proceed 5.505.50 times faster than it did at 321 K?321 K? T= 2) Consider the elementary reaction equations shown. A(g)+B(g)⟶C(g)+D(g)A(g)+B(g)⟶C(g)+D(g) 2X(g)⟶Y(g)+Z(g)2X(g)⟶Y(g)+Z(g) Write the rate law for reaction A. Write the rate law for reaction B.
Question 17 (1 point) C Determine the rate law for the following elementary reaction: H20H+OH. rate-k[H20]2 rate-k[H OH-] rate-kH 12[OH-] rate-k[H2O]
Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: rate constant elementary reaction step NO(g)+ 02(g) NO2(9) 0(g) 1 NO(g) O(g) NO2(9) k2 2 Suppose also k,»k,. That is, the first step is much faster than the second. 2* Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical reaction rate k Note: your answer should not contain the concentrations of any intermediates. Express the rate...