Question

Suppose you had a 3.25-L sample of neon gas at 21°C and a pressure of 0.954 atm. What would be the volume of this gas if the pressure were increased to 1.270 atm while the temperature remained constant?

Answer 1

Suppose you had a 3.25-L sample of neon gas at $21^{\circ}\mathrm{C}$ and a pressure of 0.954 atm. What would be the volume of this gas if the pressure were increased to 1.270 atm while the temperature remained constant?

Solution:

To find volume of neon gas if the pressure were increased to 1.270 atm while the temperature remained constant we should use the equation of combined gas law:

$$P _ {1} V _ {1} / T _ {1} = P _ {2} V _ {2} / T _ {2};$$

If the temperature remained constant the law can be written as:

$$P _ {1} V _ {1} = P _ {2} V _ {2}, T _ {1} = T _ {2} = \text {c o n s t};$$ $$V _ {1} = 3. 2 5 L = 3. 2 5 d m ^ {3} = 3. 2 5 \cdot 1 0 ^ {- 3} m ^ {3};$$ $$P _ {1} = 0. 9 5 4 \mathrm {a t m} = 0. 9 5 4 \cdot 1 0 1 3 2 5 \mathrm {P a} = 9 6 6 6 4. 0 5 \mathrm {P a};$$ $$P _ {2} = 1. 2 7 0 \mathrm {a t m} = 1. 2 7 0 \cdot 1 0 1 3 2 5 \mathrm {P a} = 1 2 8 6 8 2. 7 5 \mathrm {P a};$$ $$9 6 6 6 4. 0 5 \cdot 3. 2 5 \cdot 1 0 ^ {- 3} = 1 2 8 6 8 2 \cdot V _ {2};$$ $$V _ {2} = 2. 4 4 \cdot 1 0 ^ {- 3} m ^ {3} = 2. 4 4 d m ^ {3} = 2. 4 4 L.$$

Answer: 2.44 L