Suppose you heat an oven to 400°F (about 200°C) and boil a pot of water. Which of the following explains why you would be burned
1 answer:
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Answer: C2H6O2
Explanation: solution attached:
First convert mass to moles.
Second divide each moles on the lowest amount to find the number of atoms in the empirical formula.
Third calculate the empirical formula mass.
Fourth calculate for the molecular formula by dividing the molar mass over the empirical formula mass.
Fifth multiply the empirical formula by the answer and that is the molecular formula of the compound.
Answer:
The molar mass of the compound is:- 168.82 g/mol
The molar mass of the gas is:- 16.38 g/mol
Explanation:
(a)
Using ideal gas equation as:
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Also,
Moles = mass (m) / Molar mass (M)
Density (d) = Mass (m) / Volume (V)
So, the ideal gas equation can be written as:
Given that:-
Pressure = 20 kPa = 20000 Pa
The expression for the conversion of pressure in Pascal to pressure in atm is shown below:
P (Pa) = P (atm)
20000 Pa = atm
Pressure = 0.1974 atm
Temperature = 330 K
d = 1.23 kg/m³ = 1.23 g/L
Molar mass = ?
Applying the equation as:
0.1974 atm × M = 1.23 g/L × 0.0821 L.atm/K.mol × 330 K
⇒M = 168.82 g/mol
<u>The molar mass of the compound is:- 168.82 g/mol</u>
(b)
Given that:
Pressure = 152 Torr
Temperature = 298 K
Volume = 250 cm³ = 0.25 L
Using ideal gas equation as:
R =
Applying the equation as:
152 Torr × 0.25 L = n × 62.3637 L.torr/K.mol × 298 K
⇒n = 0.002045 moles
Given that :
Mass of the gas = 33.5 mg = 0.0335 g
Molar mass = ?
The formula for the calculation of moles is shown below:
Thus,
<u>The molar mass of the gas is:- 16.38 g/mol</u>