Question

A student sets up two reactions. reaction 1 uses 0.130 mol/l of reactant, and reaction 2 uses 0.440 mol/l of reactant. how many times faster is reaction 2 compared to reaction 1?

Answer 1

Reaction 2 is 3.385 times faster compared to reaction 1

Further explanation

The reaction rate (v) shows the change in the concentration of the substance (changes in addition to concentrations for reaction products or changes in concentration reduction for reactants) per unit time.

Can be formulated:

Reaction: aA ---> bB

$\large{\boxed{\boxed{\bold{v~=~-\frac{\Delta A}{\Delta t}}}}$

or

$\large{\boxed{\boxed{\bold{v~=~+\frac{\Delta B}{\Delta t}}}}$

A = reagent

B = product

v = reaction rate

t = reaction time

For A + B reactions ---> C + D

Reaction speed can be formulated:

$\large{\boxed{\boxed{\bold{v~=~k.[A]^a[B]^b}}}$

where

v = reaction speed, M / s

k = constant, mol¹⁻⁽ᵃ⁺ᵇ⁾. L⁽ᵃ⁺ᵇ⁾⁻¹. S⁻¹

a = reaction order to A

b = reaction order to B

[A] = [B] = concentration of substances

Reaction 1 uses 0.130 mol / l of reactant, and reaction 2 uses 0.440 mol / l of reactant.

Assuming a reaction order is one then:

reaction rate 1 =

v₁ = k. [A]

v₁ = k. 0.130

reaction rate 2 =

v₂ = k. [B]

v₂ = k. 0.440, so that

$\frac{v_2}{v_1}~=~k.\frac{0.440}{0.130}$

$\frac{v_2}{v_1}~=~3,385$

v₂ = 3.385. v₁

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Keywords: reaction rate, reaction order, molar concentration, products, reactants

Answer 2

Given:

Concentration of reactant used in reaction 1 = 0.130 mol/L

Concentration of reactant used in reaction 2 = 0.440 mol/L

To determine:

the rate of reaction 2 wrt to 1

Explanation:

Let the reaction be represented as:

Reactant → Product

Rate of reaction is:

[Rate] = k[reactant]

where k = rate constant

[reactant] = reactant concentration

for reactions 1 and 2 the rates are given as:

[Rate]₁ = k[reactant]₁=k[0.130] -------(1)

[Rate]₂= k[reactant]₂=k[0.440]--------(2)

2 ÷ 1

[Rate]₂/[Rate]₁ = 3.38

[Rate]₂ = 3.38[Rate]₁

Ans: Thus, reaction(2) is nearly 3 times faster than reaction(1)