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What is the molarity of each ion present in aqueous solutions prepared by dissolving 20.00 g of the following compounds in water to make final volumes equal to 4.5 L.a. Cobalt(III) chloride

b. Nickel(III) sulfate

c. Sodium permanganate

d. Iron(II) bromide

Answers

Answer 1

Answer:

Answer:

The molarity of Co³⁺ is 0.027 M

The molarity of Cl⁻ 0.081 M

The molarity of Ni³⁺ is 0.022 M

The molarity of SO₄²⁻ is 0.033 M

The molarity of Na⁺ is 0.031 M

The molarity of MnO₄⁻ is 0.031 M

The molarity of Fe²⁺ is 0.021 M

The molarity of Br⁻ is 0.042 M

Explanation:

The molarity of each ion is the molarity of the salt times the number of ions in the formula. First, we will calculate the molarity of each salt.

a. Cobalt(III) chloride. CoCl₃

The molar mass of CoCl₃ is 165.29 g/mol. The molarity of CoCl₃ is:

$(20.00g)/((165.29g/mol).4.5L) =0.027M$

The molarity of Co³⁺ is 1 × 0.027 M = 0.027 M

The molarity of Cl⁻ is 3 × 0.027 M = 0.081 M

b. Nickel(III) sulfate. Ni₂(SO₄)₃

The molar mass of Ni₂(SO₄)₃ is 405.57 g/mol. The molarity of Ni₂(SO₄)₃ is:

$(20.00g)/((405.57g/mol).4.5L) =0.011M$

The molarity of Ni³⁺ is 2 × 0.011 M = 0.022 M

The molarity of SO₄²⁻ is 3 × 0.011 M = 0.033 M

c. Sodium permanganate. NaMnO₄

The molar mass of NaMnO₄ is 141.92 g/mol. The molarity of NaMnO₄ is:

$(20.00g)/((141.92g/mol).4.5L) =0.031M$

The molarity of Na⁺ is 1 × 0.031 M = 0.031 M

The molarity of MnO₄⁻ is 1 × 0.031 M = 0.031 M

d. Iron(II) bromide. FeBr₂

The molar mass of FeBr₂ is 215.65 g/mol. The molarity of FeBr₂ is:

$(20.00g)/((215.65g/mol).4.5L) =0.021M$

The molarity of Fe²⁺ is 1 × 0.021 M = 0.021 M

The molarity of Br⁻ is 2 × 0.021 M = 0.042 M

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The following data were obtained in a kinetics study of the hypothetical reaction A + B + C → products. [A]0 (M) [B]0 (M) [C]0 (M) Initial Rate (10–3 M/s) 0.4 0.4 0.2 160 0.2 0.4 0.4 80 0.6 0.1 0.2 15 0.2 0.1 0.2 5 0.2 0.2 0.4 20 Using the initial-rate method, what is the order of the reaction with respect to C? a. zero-order b. first-order c. third-order d. second-order e. impossible to tell from the data given

Answers

The dependence of the power of the reaction rate on the concentration is called the order of the reaction. The order of the reaction is the first order.

What is the initial-rate method?

The initial rate method is the estimation of the order of the reaction by the initial rates of the reactants and products and by performing the reaction several times by measuring the rate.

The reaction is given as,

$\rm A + B + C \rightarrow Products$

The rate of reaction can be given as:

$\rm rate = k[A]^(x)[B]^(y)[C]^(z)$

Here the variables x, y and z are orders respective to the reactant concentration and k is the rate constant.

Value of x with respect to A:

$\begin{aligned} \rm \frac {Rate 3}{Rate 4} &= \rm [([A(3)])/([A(4)])]^(\rm x)\n\n(15)/(5) &= [([0.6])/([0.2])]^(\rm x)\n\n\rm x &= 1\end{aligned}$

Value of y with respect to B:

$\begin{aligned}\rm \frac {Rate 2}{Rate 5} &= \rm [([B(2)])/([B(5)])]^(\rm y)\n\n(80)/(20) &= [([0.4])/([0.2])]^(\rm y)\n\n\rm y &= 2\end{aligned}$

Value of z with respect to C:

$\rm \frac {Rate 1}{Rate 2} &= [([A(1)])/([A(2)])]^(x) [([B(1)])/([B(2)])]^(y) [([C(1)])/([C(2)])]^(z)$

Substituting value of x = 1 and y = 2 in the above equation:

$\begin{aligned}(160)/(80) &= [([0.4])/([0.2])]^(1)[([0.4])/([0.4])]^(2) [([0.2])/([0.4])]^(\rm z)\n\n1 &= (0.5)^(\rm z)\n\n&= 1\end{aligned}$

Therefore option b. with respect to C = 1, the order of the reaction is first-order.

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Answer:

B. First order, Order with respect to C = 1

Explanation:

The given kinetic data is as follows:

A + B + C → Products

[A]₀ [B]₀ [C]₀ Initial Rate (10⁻³ M/s)

1. 0.4 0.4 0.2 160

2. 0.2 0.4 0.4 80

3. 0.6 0.1 0.2 15

4. 0.2 0.1 0.2 5

5. 0.2 0.2 0.4 20

The rate of the above reaction is given as:

$Rate = k[A]^(x)[B]^(y)[C]^(z)$

where x, y and z are the order with respect to A, B and C respectively.

k = rate constant

[A], [B], [C] are the concentrations

In the method of initial rates, the given reaction is run multiple times. The order with respect to a particular reactant is deduced by keeping the concentrations of the remaining reactants constant and measuring the rates. The ratio of the rates from the two runs gives the order relative to that reactant.

Order w.r.t A : Use trials 3 and 4

$(Rate3)/(Rate4)= [([A(3)])/([A(4)])]^(x)$

$(15)/(5)= [([0.6])/([0.2])]^(x)$

$3 = 3^(x) \n\nx =1$

Order w.r.t B : Use trials 2 and 5

$(Rate2)/(Rate5)= [([B(2)])/([B(5)])]^(y)$

$(80)/(20)= [([0.4])/([0.2])]^(y)$

$4 = 2^(y) \n\ny =2$

Order w.r.t C : Use trials 1 and 2

$(Rate1)/(Rate2)= [([A(1)])/([A(2)])]^(x)[([B(1)])/([B(2)])]^(y)[([C(1)])/([C(2)])]^(z)$

we know that x = 1 and y = 2, substituting the appropriate values in the above equation gives:

$(160)/(80)= [([0.4])/([0.2])]^(1)[([0.4])/([0.4])]^(2)[([0.2])/([0.4])]^(z)$

$1 = (0.5)^(z)$

z = 1

Therefore, order w.r.t C = 1

A certain first-order reaction has a rate constant of 2.75 10-2 s−1 at 20.°c. what is the value of k at 45°c if ea = 75.5 kj/mol? webassign will check your answer for the correct number of significant figures. 0.0352 incorrect: your answer is incorrect.

Answers

With an activation energy $($E_a$)$ of 75.5 kJ/mol, the rate constant k for a first-order reaction at 20°C is 2.75 × 10⁻² s⁻¹. At 45°C, k is approximately 0.095 s⁻¹, determined using the Arrhenius equation.

The Arrhenius equation relates the rate constant k, temperature T, activation energy $($E_a$)$ , and the gas constant R:

$k = Ae^{-(E_a)/(RT)}$

Given that $k_1 = 2.75 * 10^(-2) \, \text{s}^(-1)$ at $T_1 = 20^\circ \text{C} = 293.15 \, \text{K}$ and $E_a = 75.5 \, \text{kJ/mol}$ , we want to find $k_2$ at $T_2 = 45^\circ \text{C} = 318.15 \, \text{K}$ .

First, let's find the value of A using the Arrhenius equation at T_1:

$2.75 * 10^(-2) = A e^{-((75.5 * 10^3))/((8.314)(293.15))}$

Solving for A:

$A \approx 3.65 \, \text{s}^(-1)$

Now, use the Arrhenius equation at $T_2$ to find $k_2$ :

$k_2 = (3.65) e^{-((75.5 * 10^3))/((8.314)(318.15))}$

Calculate $k_2$ .

$k_2 \approx 0.095 \, \text{s}^(-1)$

Therefore, the value of k at $45^\circ \text{C}$ is approximately $0.095 \, \text{s}^(-1)$ .

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Final answer:

To find the new rate constant of a first-order reaction under different temperature conditions, we can use the Arrhenius equation, which relates the rate constant, activation energy, and temperature of a reaction.

Explanation:

The student is interested in finding the value of the rate constant (k) at a different temperature for a first-order reaction. The answer can be found using the Arrhenius equation, which defines the relationship between the rate constant (k) of a reaction and the temperature at which the reaction occurs. The activation energy (Ea) is also necessary.

The Arrhenius equation is: k = A * exp(-Ea/(R*T)), where A is the pre-exponential factor, R is the universal gas constant (the value of R should be 8.314 J/mol.K to match the Ea units), and T is the temperature in Kelvin.

At the first condition, you have the value of k and the corresponding T (convert Celsius to Kelvin by adding 273.15). With these values and the known Ea, you can solve for A. Then, using the value of A, Ea, and the second T (also converted to Kelvin), you can solve for the new k.

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Pls answer this question

Answers

Answer:

A carbon dioxide and oxygen

Use the following structures of amino acids to answer the questions below. Note that the difference in the structures (the side chains) is highlighted by gray shading.

A student performed chromatography of the four amino acids and theresults were shown in the chromatogram below. If an anion exchangecolumn (column is positively charged) was used in a neutral buffer,assign each amino acid to the corresponding peak in the chromatogram.

Answers

In a positively charged column, Asparate will travel the farthest followed by Threonine, Leucine and Lysine.

The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1°C to 65.3°C?

Answers

Answer:

840.18

Explanation:

Use the equation: Q = mcΔT

m = mass (5 g)

c = specific heat (4.18)

ΔT = change in temperature (65.3-25.1 = 40.2)

$5*4.18*40.2$ = 840.12

Albus Dumbledore provides his students with a sample of 19.3 g of sodium sulfate. How many oxygen atoms are in this sample

Answers

The number of oxygen atoms in 19.3 g of sodium sulfate (Na₂SO₄) is 3.27×10²³ atoms

We'll begin by calculating the number of mole in 19.3 g of sodium sulfate (Na₂SO₄).

Mass of Na₂SO₄ = 19.3 g

Molar mass of Na₂SO₄ = (23×2) + 32 +(16×4)

= 46 + 32 + 64

= 142 g/mol

Mole of Na₂SO₄ =?

Mole = mass / molar mass

Mole of Na₂SO₄ = 19.3 / 142

Mole of Na₂SO₄ = 0.136 mole

Recall:

1 mole of Na₂SO₄ contains 4 moles of O.

Therefore,

0.136 mole of Na₂SO₄ will contain = 0.136 × 4 = 0.544 mole of O

Finally, we shall determine the number of atoms in 0.544 mole of O.

From Avogadro's hypothesis,

1 mole of O = 6.02×10²³ atoms

Therefore,

0.544 mole of O = 0.544 × 6.02×10²³

0.544 mole of O = 3.27×10²³ atoms

Thus, 19.3 g of sodium sulfate (Na₂SO₄) contains 3.27×10²³ atoms of oxygen.

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Answer:

3.27·10²³ atoms of O

Explanation:

To figure out the amount of oxygen atoms in this sample, we must first evaluate the sample.

The chemical formula for sodium sulfate is Na₂SO₄, and its molar mass is approximately 142.05 $(g)/(mol)$ .

We will use stoichiometry to convert from our mass of Na₂SO₄ to moles of Na₂SO₄, and then from moles of Na₂SO₄ to moles of O using the mole ratio; then finally, we will convert from moles of O to atoms of O using Avogadro's constant.

19.3g Na₂SO₄ · $(1 mol Na^2SO^4)/(142.05g Na^2SO^4)$ · $(4 mol O)/(1 mol Na^2SO^4)$ · $(6.022x10^2^3)/(1 mol O)$