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lukranit [14]
3 years ago
14

1. Determine the final volume of a 1.5 M HCl solution prepared from 20.0 mL

Chemistry
1 answer:
nadezda [96]3 years ago
7 0

Explanation:

Because molarity is classified as moles of solute per liter of water, dilution of the water may result in a reduction of its concentration.

Therefore, because the amount of moles of solute has to be constant for dilution, you will use the molarity and volume of that same target solution to calculate how many moles of solute will be present in the sample of the stock solution that you dilute.

c  =   \frac{n}{v}

⇒  n = c ⋅  V

n_{HCL} =  0.250 M  ⋅  6.00 L  = 1.5 moles HCl

Now all you have to do is figure out what volume of   6.0 M  stock solution will contain  1.5  moles of hydrochloric acid

c = \frac{n}{v}

V = \frac{n}{c}

V_{Stock} = \frac{1.5 moles}{6.0 \frac{moles}{L} }   = 0.25 L

Expressed in milliliters, the answer will be

V_{Stock} = 250ML →  rounded to two sig figs

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Answer:

Option D. The number of oxygen atom is the same before and after the reaction.

Explanation:

From the question given above, the following were obtained:

Robin's equation:

H₂ + O₂ —> H₂O

Alex's equation

2H₂ + O₂ —> 2H₂O

To know which equation better represents the reaction, we shall determine which of the equation is balanced.

For Robin:

H₂ + O₂ —> H₂O

Element >>> Reactant >>> Product

H >>>>>>>>> 2 >>>>>>>>>> 2

O >>>>>>>>> 2 >>>>>>>>>> 1

Robin's equation is not balanced because the number of atoms of each element in the reactant and product are not equal.

For Alex:

2H₂ + O₂ —> 2H₂O

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H >>>>>>>>> 4 >>>>>>>>>> 4

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Alex' equation is balanced because the number of atoms of each element in the reactant and product are equal.

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3 years ago
A 1.50 liter flask at a temperature of 25°C contains a mixture of 0.158 moles of methane, 0.09 moles of ethane, and 0.044 moles
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P = P1 + P2 + P3
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Explanation:

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