A 2 L bottle containing only air is sealed at a temperature of 22°C and a pressure of 0.982 atm. The bottle is placed in a freez

Answer:

The molality of the solution is 1.08 m.

Explanation:

First, determine the mass of the solvent.

A 13% solution by mass indicates that 13 grams are found in every 100 grams of solution.

Thus, solution mass = solute mass + solvent mass

100 g = 13 g + solvent mass

Therefore, solvent mass = 100 g - 13 g → 87 g

Next, we calculate the moles of solute (mass / molar mass):

13 g / 138.2 g/mol = 0.094 moles

Finally, to find the molality, which is the moles of solute per 1 kg of solvent (mol/kg), we convert the solvent mass to kg:

87 g. 1 kg / 1000 g = 0.087 kg

Then, molality → 0.094 mol / 0.087 kg = 1.08 m

Refer to the image for the answer. An aldehyde is a carbon chain that features a carbonyl group at its end, which is why it is termed aldehyde; if the carbonyl group is elsewhere on the chain, it’s referred to as a ketone. In this case, we have a 5-carbon aldehyde and the first carbon comprises the C=O group, the remaining four making up the chain. However, we must introduce a branched chain into the molecular formula. This means the longest chain cannot maintain a length of 5 carbons; instead, the maximum would be 4 carbons, making the additional carbon the branched unit. We can have two possibilities for the branched chain aldehyde with 5 carbons: one methyl group positioned at 2 and another at 3. Another potential aldehyde with branching cannot exceed 4 carbons as the longest; it must have a 3-carbon chain with 2 carbon radicals (methyl in this context). Thus, the three aldehydes with the specified formula and at least one branch can be represented, alongside their respective names in the attached image.

To address this question, utilize the molality formula, which is structured as follows:
<span>M1V1 = M2V2
You have the following values:
M1 = 2M
V1 is unknown
M2 = 0.4M
V2 = 100 ml

</span>Substituting the known values into the equation gives:
<span>2 × V1 = 0.4 × 100
</span>Thus:
V1 = 20 ml

Consequently, to prepare a total of 100 ml, you should take 20 ml of the 2 M solution and dilute it to 100 ml with water in a volumetric flask.

Volume = nRT/P

n = number of moles (particles)

R = universal gas constant (0.0821)

T = temperature (in Kelvin)

P = pressure (in atm)

(Assuming there is 1 mole of Helium involved in the chemical reaction) we need to convert grams to moles: 12.0g He x 1 mol He/4 molar mass of He = 3 mol He.

Transform Celsius to Kelvin: 100*C + 273.15 = 373.15 K.

Now we can construct the volume equation: (3mol)(0.0821)(373.15)/1.2atm = 76.6 L of Helium gas.

Answer:

• 46.6 atm

Explanation:

1) Information:

a) Volume, V = 10.0 l

b) Helium, m₁ = 48.5 g

c) Carbon dioxide, m₂ = 94.6 g

d) Temperature, T = 398 K

e) Pressure, p =?

2) Equations:

a) ideal gas law: pV = nRT

b) Moles, n: n = mass in grams / molar mass

3) Calculation:

a) Calculating moles of He:

• Atomic weight of He: 4.003 g/mol

• n₁ = 48.5 g / 4.003 g/mol = 12.12 mol

b) Calculating moles of CO₂:

• Molar weight of CO₂: 44.01 g/mol

• n₂ = 94.6 g / 44.01 g/mol = 2.15 mol

c) Total moles in the mixture:

• n = n₁ + n₂ = 12.12 mol + 2.15 mol = 14.27 mol

d) Finding Pressure, p:

• pV = nRT ⇒ p = nRT / V

• p = 14.27 mol × 0.0821 atm-l/K-mol × 398K / 10.0l = 46.6 atm