Question

Given a 1.35g sample of O2 (FM = 32.00). How many liters of volume would it have at 39oC and 879mmHg pressure?

Answer 1

Answer on Question #66271 - Chemistry – Organic Chemistry

Task:

Given a 1.35g sample of O₂ (FM = 32.00). How many liters of volume would it have at 39°C and 879mmHg pressure?

Solution:

The ideal gas law is often written as $pV = nRT$;

$$n = \frac{m}{M};$$ $$pV = \frac{m}{M}RT.$$

1) Convert all data into proper units

$$R = 0.0821 \, \text{L} \cdot \text{atm}/\text{K} \cdot \text{mol};$$ T = 39 \, ^\circ\text{C} + 273 = 312 \, \text{K}; $$P = 879 \, \text{mm Hg} \, (1 \, \text{atm}/760 \, \text{mm Hg}) = 1.1566 \, \text{atm}$$

2) We calculate now:

$$V = \frac{m(O_2)RT}{pM(O_2)};$$ $$V(O_2) = \frac{1.35 \cdot 0.0821 \cdot 312}{1.1566 \cdot 32} = 0.9343(L).$$

Answer: 0.9343 liters of O₂.

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