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3 years ago

In each pair of compounds, pick the one with the higher vapor pressure at a given temperature. Explain your reasoning.

Chemistry

1 answer:

Gnoma [55]3 years ago

8 0

Answer:

The answer is:

$PART \ A: CH_4\\\\PART \ B: CH_30H\\\\PART \ C: H_2CO$

Explanation:

Parts A:

The vapor pressure is higher in $CH_4$ because it is non-polar, while $CH_3Cl$ is polar. $CH_4$ has a lower molar weight as well.

Part B:

Although hydrogen bonding is found in both commodities, the vapor pressure is higher because of the smaller molar mass of $CH_30H$ .

Part C:

$H_2CO$ does not show hydrogen due to the increased vapor pressure

$CH_3OH$ bonding.

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Ber [7]

It is a solid 100%............

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3 years ago

Which of the following demonstrates that reactants and products are chemically different? Choose all that apply

nataly862011 [7]

Your answers would be k^+1, Cl2 and F-1

Hope this helps. Kinda winged it with my research.

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4 years ago

Read 2 more answers

If 200 grams of glucose is converted what will the total mass of ethanol and carbon dioxide be

lubasha [3.4K]

Glucose can be converted into ethanol, carbon dioxide and energy (usually in the form of heat).

Using chemical formulas, this can be illustrated as follows:
Glucose = Ethanol + Carbon Dioxide + Energy
C6H12O6 = 2C2H5OH + 2CO2 + Energy

From the periodic table:
molecular mass of carbon = 12 grams
molecular mass of oxygen = 16 grams
molecular mass of hydrogen = 1 gram

Therefore:
molar mass of glucose = 6(12) + 12(1) + 6(16) = 180 grams
molar mass of ethanol = 2(12) + 5(1) + 16 + 1 = 46 grams
molar mass of carbon dioxide = 1(12) + 2(16) = 44 grams

Based on the conversion equation, each one mole of glucose converts into two moles of ethanol and two moles of carbon dioxide.
Therefore, each 180 grams of glucose converts into 46 x 2 = 92 grams of ethanol and 44 x 2 = 88 grams of carbon dioxide in addition to energy.

To calculate the mass of ethanol and carbon dioxide produced from 200 grams of glucose, we will simply use cross multiplication as follows:
mass of ethanol = (200 x 92) / 180 = 102.2 grams
mass of carbon dioxide = (200 x 88) / 180 = 97.7 grams

Total mass of ethanol and carbon dioxide = 102.2 + 97.7 = 199.9 grams

4 0

3 years ago

a gas measured a volume 100 mL under pressure of 740 mmHg. What would the volume be under a pressure of 780 mmHg with constant t

nikdorinn [45]

Answer:

Explanation:

The new volume can be found by using the formula for Boyle's law which is

$P_1V_1 = P_2V_2$

Since we're finding the new volume

$V_2 = \frac{P_1V_1}{P_2} \\$

We have

$V_2 = \frac{100 \times 740}{780} = \frac{74000}{780} \\ = 94.8717...$

We have the final answer as

Hope this helps you

7 0

2 years ago

when 6g acetic acid is dissolved in 1000cm3 of solution then how many molecules ionize out of 1000 acetic acid molecules

iVinArrow [24]

Answer:

24.8 molecules are ionized from 1000 acetic acid molecules.

Explanation:

Acetic acid, CH₃COOH dissociates in water, thus:

CH₃COOH ⇄ CH₃COO⁻ + H⁺

Ka = 6.3x10⁻⁵ = [CH₃COO⁻] [H⁺] / [CH₃COOH]

<em>That means amount of CH₃COO⁻ (the dissociated form) that are produced is followed by the equilibrium of the weak acid.</em>

<em />

The initial molar concentration of acetic acid (Molar mass: 60g/mol) is:

6g ₓ (1mol / 60g) = 0.1 moles acetic acid, in 1000cm³ = 1L.

0.1 moles / L = <em>0.1M</em>

The 0.1M of acetic acid will dissociate producing X of CH₃COO⁻ and H⁺, thus:

[CH₃COOH] = 0.1M - X

[CH₃COO⁻] = X

[H⁺] = X

Replacing in Ka formula:

6.3x10⁻⁵ = [CH₃COO⁻] [H⁺] / [CH₃COOH]

6.3x10⁻⁵ = [X] [X] / [0.1 - X]

6.3x10⁻⁶ - 6.3x10⁻⁵X = X²

6.3x10⁻⁶ - 6.3x10⁻⁵X - X² = 0

Solving for X

X = - 0.0025 → False solution, there is no negative concentrations.

X = 0.00248M

That means, a 0.1M of acetic acid produce:

[CH₃COO⁻] = X = 0.00248M solution of the ionized form.

In a basis of 1000 molecules:

1000 molecules × (0.00248M / 0.1M) = 24.8

<h3>24.8 molecules are ionized from 1000 acetic acid molecules.</h3>

8 0

3 years ago