How do the atomic number and the mass number of an element

Electrical resistance is measured with ______________

steposvetlana [31]

Electrical resistance is measured by units of ohms.

3 0

4 years ago

Determine the rate law, including the values of the orders and rate law constant, for the following reaction using the experimen

weqwewe [10]

Answer:

Rate = (0.64 M²/min) [A]¹[B]²

Explanation:

1) Determination of the orders of A & B:

The rate law of the reaction = k [A]ᵃ[B]ᵇ

where, k is the rate law constant,

a is the order of the reaction with respect to reactant A,

b is the order of the reaction with respect to reactant B.

This is initial rate method problem:

From trial 1 & 2:

Reactant [A] has the same concentration in both trials, but [B] has different concentrations and the rate of the reaction changes, so the reaction rate depends on [B].

From trial 1, Rate₁ = k [A₁]ᵃ[B₁]ᵇ, [1.2 × 10⁻² M/min] = k [0.30 M]ᵃ[0.25 M]ᵇ

From trial 2, Rate₂ = k [A₂]ᵃ[B₂]ᵇ, [4.8 × 10⁻² M/min] = k [0.30 M]ᵃ[0.50 M]ᵇ

By dividing Rate₁ / Rate₂:

Rate₁ / Rate₂ = k [A₁]ᵃ[B₁]ᵇ / k [A₂]ᵃ[B₂]ᵇ

[1.2 × 10⁻² M/min] / [4.8 × 10⁻² M/min] = k [0.30 M]ᵃ[0.25]ᵇ / k [0.30 M]ᵃ[0.50 M]ᵇ

0.25 = [0.50]ᵇ

Taking log for both sides; log(0.25) = b log(0.5)

b = log(0.25) / log(0.5) = 2.

The reaction is second order with respect to reactant B.

By the same way for reactant A:

From trial 2 & 3:

Reactant [B] has the same concentration in both trials, but [A] has different concentrations and the rate of the reaction changes, so the reaction rate depends on [A].

From trial 2, Rate₂ = k [A₂]ᵃ[B₂]ᵇ, [4.8 × 10⁻² M/min] = k [0.30 M]ᵃ[0.50 M]ᵇ

From trial 2, Rate₃ = k [A₃]ᵃ[B₃]ᵇ, [9.6 × 10⁻² M/min] = k [0.60 M]ᵃ[0.50 M]ᵇ

By dividing Rate₂ / Rate₃:

Rate₂ / Rate₃ = k [A₂]ᵃ[B₂]ᵇ / k [A₃]ᵃ[B₃]ᵇ

[4.8 × 10⁻² M/min] / [9.6 × 10⁻² M/min] = k [0.30 M]ᵃ[0.50 M]ᵇ / k [0.60 M]ᵃ[0.50 M]ᵇ

0.50 = [0.50]ᵃ

Taking log for both sides; log(0.50) = a log(0.5)

a = log(0.50) / log(0.50) = 1.

The reaction is first order with respect to reactant A.

The rate law of the reaction will be: Rate = k [A]¹[B]²

The overall order of the reaction is third order reaction.

2) Determining the rate law constant:

Taking data of trial 1:

Rate = k [A]¹[B]²

[1.2 × 10⁻² M/min] = k [0.30 M]¹[0.25 M]²

k = [1.2 × 10⁻² M/min] / [0.30 M]¹[0.25 M]² = 0.64 M²/min.

So, the rate law will be: Rate = (0.64 M²/min) [A]¹[B]²

3 0

3 years ago

Cadmium metal reacts with a nickel (III) chlorate solution

DochEvi [55]

Nickel metal reacts with cadmium(II) nitrate reacts to produce cadmium metal and nickel(Il) nitrate Write the reaction equation on your scratch paper before answering this question. For this reaction Ni is the reducing agent and gains electrons_ Cd2' is the oxidizing agent and it loses electrons Cd?" is the reducing agent and it loses electrons Cd2" is the oxidizing agent and it gains electrons Ni is the oxidizing agent and it loses electrons

4 0

2 years ago

Cual es punto de congelacion del agua

Marianna [84]

nao sei mas

Explanation:

6 0

3 years ago

Please help with this chemistry question, image attached.

Alexeev081 [22]

Answer:

a. Sally did not take account the atoms of the compounds, because she only summed Al + O and in the oxide, we have 2 mol of Al and 3 mol of O

b. The conversion factor that Jacob did, was wrong.

Moles must be divided by moles, so they can be cancelled. The correct conversion factor is:

9.45 mol . 102 g / 1 mol = 963.9 g

Explanation:

Al₂O₃ → Aluminum oxide

We determine the molar mass:

Molar mass Al . 2 + Molar mass O . 3

27 g/mol . 2 + 16 g/mol . 3 = 102 g/mol

a. Sally did not take account the atoms of the compounds, because she only summed Al + O and in the oxide, we have 2 mol of Al and 3 mol of O

b. The conversion factor that Jacob did, was wrong.

Moles must be divided by moles, so they can be cancelled. The correct conversion factor is:

9.45 mol . 102 g / 1 mol = 963.9 g

7 0

3 years ago