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Masja [62]
3 years ago
5

It is required to prepare 1250 kg of a solution composed of 12 wt.% ethanol and 88 wt.% water. Two solutions are available, the

first contains 5 wt.% ethanol, and the second contains 25 wt.% ethanol. How much of each solution are mixed to prepare the desired solution?
Chemistry
1 answer:
bekas [8.4K]3 years ago
8 0

Answer:

437.5 kg of first solution and 812.5 kg of second solution should be mixed to get desired solution.

Explanation:

Let the mass of the first solution be x and second solution be y.

Amount solution required = 1250 kg

x + y = 1250 kg....[1]

Percentage of ethanol in required solution = 12% of 1250 kg

Percentage of ethanol in solution-1 = 5% of x

Percentage of ethanol in required solution = 25% of y

5% of x +  25% of y =12% of 1250 kg

\frac{5}{100}\times x+\frac{25}{100}y=\frac{12}{100}\times 1250 kg

x + 5y = 3000 kg...[2]

Solving [1] and [2] we :

x = 437.5 kg   , y =  812.5 kg

437.5 kg of first solution and 812.5 kg of second solution should be mixed to get desired solution.

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To find the pressure of the cylinder, we need to find moles of gas produced, and using general gas law we can determine the pressure of the gas:

<em>Moles Pb(NO₃)₂ and moles of gas:</em>

3.31g * (1mol / 331g) = 0.01 moles of Pb(NO₃)₂.

That means moles of gas produced is 0.05 moles.

<em>Pressure of the gas:</em>

Using PV = nRT

P = nRT/V

<em>Where P is pressure (Incognite)</em>

<em>V is volume (2.53L)</em>

<em>R is gas constant (0.082atmL/molK)</em>

<em>T is absolute temperature (300K)</em>

And n are moles of gas (0.05 moles)

P = 0.05mol*0.082atmL/molK*300K / 2.53L

P = 0.486atm is the pressure of the cylinder

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The given reaction is:

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H = 10                                  H = 2

O = 2                                   O = 3

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5 0
2 years ago
5.11 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the
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Explanation:

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q=mc\Delta T

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q = heat absorbed by water = ?

m = mass of water = {\text {volume of water}}\times {\text {density of water}}=100.0ml\times 1.00g/ml=100.0g

c = heat capacity of water = 4.186 J/g°C

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