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Westkost [7]
3 years ago
7

Percentage of isotopes in 35/17 Cl and 37/17 Cl with the molar mass of chlorine as 35.5g and the mass of each nucleon to be 1.00

00 amu
Chemistry
1 answer:
AlekseyPX3 years ago
4 0

Answer:

The abundance of 35/17 Cl is 75% and 25% of 37/17Cl

Explanation:

The molar mass of an atom is defined as the sum of the masses of each isotope times its abundance, that is:

35.5amu = 35amu*X + 37amu*Y <em>(1)</em>

<em>Where X is the abundance of the 35/17Cl and Y the abundance of 37/17 Cl</em>

<em />

As there are just these 2 isotopes and the abundances of both isotopes = 1:

X + Y = 1 <em>(2)</em>

<em></em>

Replacing (2) in (1):

35.5 = 35X + 37(1-X)

35.5 = 35X + 37 - 37X

-1.5 = -2X

X = 0.75 = 75%

And Y = 100-75% = 25%

<h3>The abundance of 35/17 Cl is 75% and 25% of 37/17Cl</h3>
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Answer:

Explanation:

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What do you notice about the elements on the reactant and product side of the equation
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A bottle of a commercial reagent-grade hydrochloric acid, HCI, has the following
Doss [256]

The volume of concentrated HCl : 2.073 ml

<h3>Further explanation</h3>

Given

37% HCl by mass; density 1.19 g/mL

Required

The volume of concentrated HCl

Solution

Conversion to molarity :

37% x 1.19 g/ml =0.4403 g/ml

g/ml to mol/L :

=0.4403 g/ml x 1000 ml/L : 36.5 g/mol

=12.06 mol/L

or we can use formula :

\tt M=\dfrac{\%\times \rho\times 10}{MM}\\\\M=\dfrac{37\times 1.19\times 10}{36.5}\\\\M=12.06

Dilution formula :

M₁V₁=M₂V₂

12.06 M x V₁ = 0.1 M x 0.25 L

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4 0
2 years ago
Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it
kvasek [131]

Answer:

0.396 M

Explanation:

Let's consider the following reaction.

2 COF₂(g) ⇌ CO₂(g) + CF₄(g)

We can find the concentrations at equilibrium using an ICE Chart.

         2 COF₂(g) ⇌ CO₂(g) + CF₄(g)

I            2.00              0            0

C           -2x                +x          +x

E         2.00-2x            x             x

The concentration equilibrium constant (Kc) is:

Kc=4.10=\frac{[CO_{2}][CF_{4}]}{[COF_{2}]^{2} } =\frac{x^{2} }{(2.00-2x)^{2} } =(\frac{x}{2.00-2x} )^{2} \\\sqrt{4.10} = \frac{x}{2.00-2x}\\4.05-4.05x=x\\x=0.802

The concentration of COF₂ at equilibrium is:

[COF₂] = 2.00-2x = 2.00-2(0.802) = 0.396 M

4 0
3 years ago
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