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Paha777 [63]
3 years ago
8

A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq) , until no further precipitation occurs. The

precipitate is collected by filtration, dried, and weighed. A total of 18.86 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.
Chemistry
1 answer:
Hoochie [10]3 years ago
7 0

<u>Answer:</u> The molarity of Pb(NO_3)-2 solution is 0.34 M.

<u>Explanation:</u>

  • To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

<u>For lead chloride:</u>

Given mass of lead chloride = 18.86 g

Molar mass of lead chloride = 278.1 g/mol

Putting values in above equation, we get:

\text{Moles of lead chloride}=\frac{18.86g}{278.1g/mol}=0.068mol

  • For the balanced chemical equation:

Pb(NO_3)_2+2NaCl\rightarrow PbCl_2+2NaNO_3

By Stoichiometry of the reaction:

1 mole of lead chloride is formed by 1 mole of lead nitrate

So, 0.068 moles of lead chloride will be formed from = \frac{1}{1}\times 0.068=0.068mol of lead nitrate

  • To calculate the molarity of solution, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}

We are given:

Volume of solution = 200 mL = 0.200 L   (Conversion factor: 1 L = 1000 mL)

Moles of lead nitrate = 0.068 moles

Putting values in above equation, we get:

\text{Molarity of }Pb(NO_3)_2\text{ solution}=\frac{0.068mol}{0.065L}\\\\\text{Molarity of }Pb(NO_3)_2\text{ solution}=0.34M

Hence, the molarity of Pb(NO_3)-2 solution is 0.34 M.

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Answer:

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Explanation:

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Which of the following represents the mass of 1 molecule of SH2?
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Answer:
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Solution:

Step 1) Calculate Molar Mass of SH₂;

Atomic Mass of Sulfur    =  32 g/mol

Atomic Mass of H₂         =  2 g/mol
                                      --------------------
Molecular Mass of SH₂  =  34 g/mol

Step 2: Calculate mass of one molecule of SH₂ as;

As,

                     Moles  =  # of Molecules / 6.022 × 10²³

Also, Moles  =  Mass / M.Mass So,

                     Mass/M.mass  =  # of Molecules / 6.022 × 10²³

Solving for Mass,

                     Mass  = # of Molecules × M.mass / 6.022 × 10²³

Putting values,

                     Mass  =  (1 Molecule × 34 g.mol⁻¹) ÷ 6.022 × 10²³

                     Mass  =  5.645 × 10⁻²³ g
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Darwin's theorized that three conditions were necessary for natural selection to occur, which of the following is NOT one of the
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Answer:

The correct option is: stable environment

Explanation:

According to the Darwin's theory, natural selection is the concept by which all the small useful variations of traits are preserved.

According to Darwin, there are three <u>necessary and sufficient conditions</u> for the occurrence of natural selection:

1. struggle for existence

2. variation

3. inheritance

These conditions are said to be necessary because if these conditions are not satisfied then natural selection does not occur.

These conditions are said to be sufficient because if these conditions are satisfied, then natural selection will most definitely occur.

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Answer:

10 moles of SO₂ are produced when 5 moles of FeS₂

Explanation:

Stoichiometry: it is the theoretical proportion in which the chemical species are combined in a chemical reaction. The stoichiometric equation of a chemical reaction relates molecules or number of moles of all the reagents and products that participate in the  reaction.

In other words, stoichiometry establishes relationships between the molecules or elements that make up the reactants of a chemical equation with the products of said reaction. The relationships established are molar relationships (that is, moles) between the compounds or elements that make up the chemical equation.

The stoichiometric coefficients of a chemical reaction indicate the proportion in which said substances react.

Taking into account the above, you can apply the following rule of three: by stoichiometry if 4 moles of FeS₂ produce 8 moles of SO₂, then when reacting 5 moles of FeS₂ how many moles of SO₂ will they produce?

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