Answer:
Molar mass = 32.64 g / mol.
The density of gas is 1.3 × 10⁻³g/mL.
Explanation:
Given data:
Mass of sample = 2.35 g
Pressure = 1.05 atm
Volume = 1.85 L (1.85 × 1000 = 1850 ml)
Temperature = 55 °C (55+ 273.15 = 328.15 K)
Density = ?
Formula:
d = m/ v
The volume of flask would be the volume of gas.
d = 2.35 g / 1850 mL = 0.0013 g/mL or 1.3 × 10⁻³g/mL
The density of gas is 1.3 × 10⁻³g/mL.
Molar mass:
Now we will calculate the moles of a gas first in order to find the molar mass of a gas.
Formula:
PV =nRT
n = number of moles.
n = PV / RT
n = 1.05 atm × 1.85 L / 0.0821 atm. dm³. K⁻¹ . mol⁻¹ × 328.15 K
n = 1.9425 atm . L / 26.941115 atm . dm.³mol⁻¹
n = 0.072 mol
Now we will find the molar mass.
Number of moles = mass / molar mass
0.072 mol = 2.35 g / molar mass
Molar mass = 2.35 g / 0.072 mol
Molar mass = 32.64 g / mol
The mole ratio can be seen below and the volume of each precipitate is 60 mL.
A mole ratio refers to a conversion factor that compares the quantities of two chemicals in moles in a chemical laboratory experiment.
<u>Mole ratio For 1:</u>
- = 10 mL : 50 mL
- = 1 : 5 mL
<u>Mole ratio For 2:</u>
<u>Mole ratio For 3:</u>
<u>Mole ratio For 4:</u>
<u>Mole ratio For 5:</u>
<u>Mole ratio For 6:</u>
<u>Mole ratio For 7:</u>
Since the parameters from the left side of the diagram are not shown, we will assume that the volumes for each precipitate are the addition of both volumes in each column.
By doing so, we have:
1.
2.
3.
4.
5.
6.
7.
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Answer:
A). It encouraged them to rely on observation and experimentation to support their conclusions.
Explanation:
