Can water (or any solvent) dissolve an infinite amount of solute?

the energy to break 1 mol of C-C bonds is 348 kj/mol. what would be the minimum frequency of a single photon that would break a

mr_godi [17]

Answer:

f = 5.25 x 10³⁸ s⁻¹

Explanation:

Energy = 348KJ = 348,000 J

Frequency = ?

Energy and frequency are related by the equation below;

E = hf

where h = Planck's constant = (6.626 x 10-34 J · s),

Upon making f subject of formular;

f = E / h

substituting the values, we have;

f = 348,000 / 6.626 x 10-34

f = 52,520 x 10 ³⁴ s⁻¹

f = 5.25 x 10³⁸ s⁻¹

4 0

2 years ago

Item 5 A solution of methanol, CH3OH, in water is prepared by mixing together 128 g of methanol and 108 g of water. The mole fra

Basile [38]

Answer:

Mole fraction of methanol will be closest to 4.

Explanation:

Given, Mass of methanol = 128 g

Molar mass of methanol = 32.04 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{128\ g}{32.04\ g/mol}$

$Moles\ of\ methanol = 3.995\ mol$

Given, Mass of water = 108 g

Molar mass of water = 18.0153 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{108\ g}{18.0153\ g/mol}$

$Moles\ of\ water= 5.995\ mol$

So, according to definition of mole fraction:

$Mole\ fraction\ of\ methanol=\frac {n_{methanol}}{n_{methanol}+n_{water}}$

$Mole\ fraction\ of\ methanol=\frac{3.995}{3.995+5.995}=0.39989$

<u>Mole fraction of methanol will be closest to 4.</u>

5 0

2 years ago

Click the "draw structure" button to launch the drawing utility. Propane (CH3CH2CH3) has both 1° and 2° hydrogens. Draw the carb

OlgaM077 [116]

Answer:

a) find attached image 1

b) find attached image 2

Explanation :

The more stable radical is formed by a reaction with smaller bond dissociation energy.

since the bond dissociation for cleavage of the bond to form primary free radical is higher, more energy must be added to form it. This makes primary free radical higher in energy and therefore less stable than secondary free radical.

6 0

2 years ago

For each pair below, select the sample that contains the largest number of moles. Pair A 2.50 g O2 2.50 g N2

raketka [301]

Answer:

Explanation:

Pair 2.50g of O₂ and 2.50g of N₂

The atoms sample with the largest number of moles since the masses are the same would be the one with lowest molar mass according the the equation below:

Number of moles = $\frac{mass }{molarmass}$

Atomic mass of O = 16g and N = 14g

Molar mass of O₂ = 16 x 2 = 32gmol⁻¹

Molar mass of N₂ = 14 x 2 = 28gmol⁻¹

Number of moles of O₂ = $\frac{2.5}{32}$ = 0.078mole

Number of moles of N₂ = $\frac{2.5}{28}$ = 0.089mole

We see that N₂ has the largest number of moles

4 0

2 years ago

Read 2 more answers

Butyl butyrate is an ester that is a naturally occurring oil used in the flavor industry for its fruity scent. If the steam dist

Snezhnost [94]

Answer:

The correct answer is 62.5 %.

Explanation:

Based on the given information, the partial pressure of butyl butyrate is 50 mmHg and the partial pressure of water is 710 mmHg.

Hence, the total pressure is 710+50 = 760 mmHg

According to Dalton's law of partial pressure,

Partial pressure = mole fraction * total pressure

Mole fraction of water is,

Partial pressure of water/Total pressure = 710/760 = 0.93

Similarly, the mole fraction of butyl butyrate is,

Partial pressure of butyl-butyrate/Total pressure = 50/760 = 0.07

Therefore, mole% of water is 0.93 * 100 = 93 %

For calculating mass%,

Mass of H2O = 0.93 * 18 = 16.8 grams (The molecular mass of water is 18 grams per mole)

The molecular mass of butyl-butyrate is 144 gram per mole

The mass of butyl-butyrate = 144 * 0.07 = 10.08 grams

The mass percent of water will be,

Mass % of water/Total mass % * 100 = 16.8 / 10.08 + 16.8 * 100 = 62.5%.

8 0

2 years ago