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3 years ago

What typically occurs in a substance where hydrogen bonding exists when compared to the same substance without H-bonds?

Chemistry

1 answer:

djverab [1.8K]3 years ago

7 0

Answer:

B) Increase in boiling point and decrease in vapor pressure

Explanation:

Vapor pressure is inversely related to the Boiling point , as

higher the boiling point, lower the vapor pressure. and

Lower the boiling point, higher the vapor pressure.

Hydrogen bonding.

The electrostatic attraction between Hydrogen , bonded to electronegative atom like F, O, N and the more electronegative atom is called as Hydrogen bonding.

For example -

In alcohols, - OH group has Hydrogen that is bonded to more electronegative atom O.

As ,

Extra energy is required to break Hydrogen bonds.

because the substance which exhibits Hydrogen bonding have lower vapor pressure than that of the substance with out Hydrogen bonding.

Hence , the substance with Hydrogen bonding , has higher boiling point,.

Hence , the correct option is Increase in boiling point and decrease in vapor pressure .

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2. What is the molarity of a HCl solution containing 1.2 grams of hydrochloric acid in 0.025 L of solution?

alisha [4.7K]

Answer:

1.3M

Explanation:

Convert from grams to moles:

molar mass of HCl = 1.01g(molar mass of H) + 35.45g(molar mass of Cl) = 36.46g HCl

1.2g HCl (1mol HCl/36.46g HCl)

= .0329 mol HCl

Molarity = mol/L (important formula for concentration)

Plug your values in:

Molarity = .0329mol/.025L

1.317M - but you used two significant figures in the question, so:

1.3M

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3 years ago

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2 years ago

When aqueous solutions of Na2SO4 and Pb(NO3)2 are mixed, PbSO4 precipitates. Calculate the mass of PbSO4 formed when 1.25 L of 0

neonofarm [45]

Answer:

The mass of PbSO4 formed 15.163 gram

Explanation:

mole of Pb(NO₃)₂ = 1.25 x 0.05 = 0.0625

mole of Na₂SO₄ = 2 x 0.025 = 0.05

Pb(NO₃)₂ + Na₂SO₄ → PbSO₄ + 2 NaNO₃

( Mole/Stoichiometry ) $\frac{0.0625}{1}$ $\frac{0.05}{1}$

= 0.0625 = 0.05

From (Mole/ Stoichiometry ) we can conclude that Na₂SO₄ is limiting reagent.

Mass of PbSO₄ precipitate = 0.05 x Molecular mass of PbSO₄

= 0.05 x 303.26 g

= 15.163 g

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3 years ago

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containi

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3 years ago

It is desired to produce 2.25 grams of dichloromethane (CH2Cl2) by the following reaction. If the percent yield of dichlorometha

Allushta [10]

Answer:- 3.12 g carbon tetrachloride are needed.

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$CH_4+CCl_4\rightarrow 2CH_2Cl_2$

From given actual yield and percent yield we will calculate the theoretical yield that would be further used to calculate the grams of carbon tetrachloride.

percent yield formula is:

percent yield = $(\frac{actual}{theoretical})100$