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Natalija [7]
3 years ago
6

200.0 mL OF A 5.10 M solution are diluted to 500.0 mL. What is the concentration of the resulting solution? *

Chemistry
2 answers:
erastova [34]3 years ago
3 0

Answer:

Concentration of the resulting solution = 2.04 M

Explanation:

<u>Data:</u>

M1 = 5.10 M

V1 = 200.0 mL

V2 = 500.0 mL

M2 = ?

By modifying the volume of solution, keeping the amount of solute constant, the concentration changes. To perform the calculations, the equation will be:

M1*V1=M2*V2

Where M1 is the initial concentration of the solution, M2 the final concentration and V is the value of the volumes of the initial and final solution.

Clearing the value of M2 from the equation and replacing the values ​​we have:

M2=\frac{M1*V1}{V2} =\frac{5.10M*200mL}{500mL} =2.04M

vazorg [7]3 years ago
3 0

Answer:

2.04M

Explanation:

Using C1V1 = C2V2

where;

C1 =  Concentration of stock solution  = 5.10M

C2 = Final concentration of new solution = x

V1 = Volume of stock solution = 200ml

V2 = Final volume of new solution = 500ml

Inserting the values into the formulae, we have;

5.10 * 200 = x * 500

x = (5.10 * 200) / 500

x = 2.04M

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Answer:

See explanation

Explanation:

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Sodium reacts with cold water to give a vigorous reaction,magnesium and aluminium reacts with steam at red heat.

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8 0
2 years ago
Dinitrogen pentoxide is used in the preparation of explosives. If 7.93 mol of
Tpy6a [65]

The volume of O₂ produced: 84.6 L

<h3>Further explanation</h3>

Given

7.93 mol of  dinitrogen pentoxide

T = 48 + 273 = 321 K

P = 125 kPa = 1,23365 atm

Required

Volume of O₂

Solution

Decomposition reaction of dinitrogen pentoxide

2N₂O₅(g)→4NO₂(g)+O₂ (g)

From the equation, mol ratio N₂O₅ : O₂ = 2 : 1, so mol O₂ :

= 0.5 x mol N₂O₅

= 0.5 x 7.93

= 3.965 moles

The volume of O₂ :

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5 0
3 years ago
A naturally occurring oil co-distills with water to produce an oil/water distillate that is 20% oil by weight. If the molecular
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Answer:

Explanation:

Partial pressure of oil = mole fraction of oil x total pressure

mole fraction of oil = mole of oil / mole of water + mole of oil

= mole of oil = mass of oil / molecular weight of oil

= 20 / 100 = .2

mole of water = 80 / 18

= 4.444

mole fraction of oil =  .2 / .2 + 4.444

= .2 / 4.644

Partial pressure of oil = mole fraction of oil x total pressure

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3 0
3 years ago
calculate the heat required in joules to convert 18.0 grams of water ice at a temperature of -20 c to liquid water at the normal
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Answer:

Explanation:

Heat required to convert ice to ice at 0⁰C

= mass x specific heat x rise in temperature

= 18 x 2.09 x 20

= 752.4 J .

heat required to convert ice at 0⁰C to water at 0⁰C

mass x latent heat of fusion

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= 6048 J

Heat required to increase the temperature of water to 100⁰C

= 18 x 4.2 x 100

= 7560 J

Total heat required

7560 + 6048 + 752.4

= 14360.4 J

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2 years ago
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