Question

The effect of chlorofluorocarbons (such as CCl₂F₂) on the depletion of the ozone layer is well known. The use of substitutes, such as CH₃CH₂F(g), for the chlorofluorocarbons, has largely corrected the problem. Calculate the volume occupied by 10.0 g of each of these compounds at STP:

a) CCl₂F₂: 5.6 L, CH₃CH₂F(g): 3.4 L
b) CCl₂F₂: 3.4 L, CH₃CH₂F(g): 5.6 L
c) CCl₂F₂: 7.2 L, CH₃CH₂F(g): 2.2 L
d) CCl₂F₂: 2.2 L, CH₃CH₂F(g): 7.2 L

Answer 1

The calculation of the volume occupied by 10.0 g of both CCl₂F₂ and CH₃CH₂F(g) at STP reveals that none of the answer options provided (a, b, c, d) match the calculated volumes of 1.85 L for CCl₂F₂ and 4.66 L for CH₃CH₂F(g). Therefore, there may be an error in the provided options.

Step-by-step explanation:

The question pertains to the calculation of the volume occupied by two chemicals, CCl₂F₂ and CH₃CH₂F(g), each weighing 10.0 g, at standard temperature and pressure (STP). The volume can be determined using the ideal gas law PV=nRT and the molar volumes of gases at STP. The molar mass of CCl₂F₂ is 120.91 g/mol, and for CH₃CH₂F(g), it is 48.06 g/mol. Using Avogadro's principle, we know that 1 mole of any gas at STP occupies 22.4 liters.

For CCl₂F₂:
(10.0 g) / (120.91 g/mol) = 0.0827 moles.
Total volume = 0.0827 moles × 22.4 L/mol = 1.85 L.

For CH₃CH₂F(g):
(10.0 g) / (48.06 g/mol) = 0.208 moles.
Total volume = 0.208 moles × 22.4 L/mol = 4.66 L.

Since the options provided do not match our calculations, it's possible that there may have been a mistake in the question or in the options listed.