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Rashid [163]
2 years ago
14

which method would be best for separating the compounds of a mixture that is made from two diffrent liquids

Chemistry
1 answer:
kobusy [5.1K]2 years ago
5 0

Answer:

fractional distillation since ot depends on the different liquids to have different boiling points

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a concentration solution of H2so4 is 59.4% by mass (m/m) and has a density of 1.83 g/mL. How many mL of the solution would be re
Blababa [14]

Answer: 41.5 mL

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

Molarity=\frac{n}{V_s}

where,

n = moles of solute

V_s = volume of solution in L

Given : 59.4 g of H_2SO_4 in 100 g of solution  

moles of H_2SO_4=\frac{\text {given mass}}{\text {molar mass}}=\frac{59.4g}{98g/mol}=0.61

Volume of solution =\frac{\text {mass of solution}}{\text {density of solution}}=\frac{100g}{1.83g/ml}=54.6ml

Now put all the given values in the formula of molality, we get

Molality=\frac{0.61\times 1000}{54.6ml}=11.2M

To calculate the volume of acid, we use the equation given by neutralisation reaction:

M_1V_1=M_2V_2

where,

M_1\text{ and }V_1 are the molarity and volume of stock acid which is H_2SO_4

M_2\text{ and }V_2 are the molarity and volume of dilute acid which is H_2SO_4

We are given:

M_1=11.2M\\V_1=mL\\M_2=0.30M\\V_2=1550mL

Putting values in above equation, we get:

11.2\times V_1=0.30\times 1550\\\\V_1=41.5mL

Thus 41.5 mL of the solution would be required to prepare 1550 mL of a .30M solution of the acid

4 0
3 years ago
A 50.0 N force is applied to an object travels with a constant velocity of 20m/s, calculate
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Explanation:

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7 0
3 years ago
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If the pressure in the room is 759.2 torr and the vapor pressure of water is 23.8 torr, what is the pressure of hydrogen gas in
Gwar [14]

The partial pressure of Hydrogen gas can directly be calculated by simply taking the difference of the overall pressure and the vapour pressure of water. That is:

 

P (H2 gas) = 759.2 torr – 23.8 torr

<span>P (H2 gas) = 735.4 torr</span>

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3 years ago
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