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11Alexandr11 [23.1K]
3 years ago
9

A chemist wishes to decrease the vapor pressure of a large volume of water. Which amount of solute will decrease it the most? (N

ote: Assume each sample of solute completely dissolves in the water.)
A)0.10 mol Al2(SO4)3

B)0.10 mol sucrose

C)0.40 mol glucose

D)0.20 mol NaCl
Chemistry
2 answers:
Vladimir79 [104]3 years ago
8 0

Answer: A) 0.10 mol Al_2(SO_4)_3

Explanation:

As the relative lowering of vapor pressure is directly proportional to the amount of dissolved solute.

The formula for relative lowering of vapor pressure will be,

\frac{p^o-p_s}{p^o}=i\times x_2

where,

\frac{p^o-p_s}{p^o}= relative lowering in vapor pressure

i = Van'T Hoff factor  

x_2 = mole fraction of solute

1. For 0.10 mol Al_2(SO_{4})_3

Al_2(SO_4)_3\rightarrow 2Al^{3+}+3SO_4^{2-}  

, i= 5 as it is a electrolyte and dissociate to give 5 ions. and concentration of ions will be 2\times 0.1+3\times 0.1=0.5

2.  For 0.10 mol sucrose

, i= 1 as it is a non electrolyte and does not dissociate, concentration of ions will be 1\times 0.1=0.1

3. For 0.40 mol glucose

, i= 1 as it is a non electrolyte and does not dissociate,  concentration of ions will be 1\times 0.4=0.4

4. For 0.2 NaCl

NaCl\rightarrow Na^{+}+Cl^{-}  

, i= 2 as it is a electrolyte and dissociate to give 2 ions, concentration of ions will be 1\times 0.2+1\times 0.2=0.4

Thus as concentration of solute is highest for Al_2(SO_4)_3 , the vapor pressure will be lowest.

valentinak56 [21]3 years ago
5 0

Answer:c

Explanation:

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Consider the balanced equation below. 4NH3 + 3O2 --> 2N2 + 6H2O What is the mole ratio of NH3 to N2?
AURORKA [14]
The balanced equation given is:
4NH3 + 3O2 .....> 2N2 + 6H2O

From this equation, we can note that 4 moles of NH3 are required to produce 2 moles of N2.

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In which state of matter is there no particle movement

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8 0
3 years ago
Extra Stoichiometry Practice
Irina-Kira [14]

Answer: 50. 4g

Explanation:

First calculate number of moles of aluminium in 38.8g

Moles = 38.8g/ 26.982mol/g

= 1.44mol

By looking at the balance equation you can see that 4 moles of aluminium produce 2 moles of aluminium oxide.

4 = 2

1.4 = x

Find the value of x

x= (1.4×2)/4= 0.72 mol

0.72 moles of aluminium oxide are produced from 38.8g of aluminium

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2 years ago
Mn2+
snow_lady [41]

The molarity of the stock Mn²⁺ ions is 0.0288 M

Based on the dilution formula;

  • The molarity of A is 0.00144 M
  • The molarity of B is 0.0000576 M
  • The molarity of C is 0.000001152 M

<h3>What is the molarity of a solution?</h3>

The molarity of a solution is the number of moles of a solute dissolved in a given volume of solution in liters.

  • Molarity = number of moles/volume

The molarity of the stock solution is:

moles of Mn²⁺ ions = mass / molar mass

molar mass of  Mn²⁺ ions = 55.0 g/mol

moles of Mn²⁺ ions = 1.584 / 55

moles of Mn²⁺ ions = 0.0288 moles

molarity of Mn²⁺ ions = 0.0288 / 1

molarity of Mn²⁺ ions = 0.0288 M

The dilution formula is used to determine the molarities of A, B, and C.

C₁V₁ = C₂V₂

C₂ = C₁V₁ / V₂

Where;

  • C₁ = initial molarity
  • V₁ = initial volume
  • C₂ = final molarity
  • V₂ = final volume

Molarity of A = 50 * 0.0288 / 1000

Molarity of A = 0.00144 M

Molarity of B = 10 * 0.00144 / 250

Molarity of B = 0.0000576 M

Molarity of C = 10 * 0.0000576 / 500

Molarity of C = 0.000001152 M

Learn more about molarity at: brainly.com/question/17138838

#SPJ1

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