Boyle’s Law-Related Problem

Boyle’s law states that the quantity of a perfect gas is inversely proportional to its absolute pressure at a constant temperature. The laws are often expressed as an equation in a few alternative ways. PV = k, where P denotes pressure, V denotes volume, and k denotes a continuing. When the temperature is kept constant, the rule can also be wont to determine the pressure or volume of a system:

PiVi = PfVf, 

where, 

Pi = initial pressure

Vi = initial volume

Pf = final pressure

Vf = final volume

Boyle’s law-related Problem 

1: A gas occupies 12.3 litres at a pressure of 40.0 mmHg. What’s the quantity when the pressure is increased to 60.0 mmHg?

(40.0 mmHg) (12.3 litres) = (60.0 mmHg) (x)

x = 8.20 L

Note three significant figures.

2: If a gas at 25.0 °C occupies 3.60 litres at a pressure of 1.00 atm, what will be its volume at a pressure of two .50 atm?

(1.00 atm) ( 3.60 litres) = (2.50 atm) (x)

x = 1.44 L

3: To what pressure must a gas be compressed to push into a 3.00 cu ft tank the whole weight of a gas that occupies 400.0 cu. ft. at standard pressure?

(400.0 cu. ft) (1.00 atm) = (x) (3.00 cu ft)

x = 133 atm

It doesn’t matter what the quantity units are. It just matters that they be an equivalent on all sides .

4: A gas occupies 1.56 L at 1.00 atm. what is going to be the quantity of this gas if the pressure becomes 3.00 atm?

(1.56 L) (1.00 atm) = (3.00 atm) (x)

 x=0.520 L

5: A gas occupies 11.2 litres at 0.860 atm. What’s the pressure if the quantity becomes 15.0 L?

(11.2 litres) (0.860 atm) = (x) (15.0 L)

x = 0.642 atm

6: 500.0 mL of gas is collected at 745.0 mmHg. What is going to be the quantity at standard pressure?

(745.0 mmHg) (500.0 mL) = (760.0 mmHg) (x)

x = 490.1 mL

7: Convert 350.0 mL at 740.0 mmHg to its new volume at standard atmosphere .

(740.0 mmHg) (350.0 mL) = (760.0 mmHg) (x)

8: Convert 338 L at 63.0 atm to its new volume at standard atmosphere .

(63.0 atm) (338 L) = (1.00 atm) (x)

9: Convert 273.15 mL at 166.0 kPa to its new volume at standard atmosphere .

(166.0 kPa) (273.15 mL) = (101.325 kPa) (x)

10: Convert 77.0 L at 18.0 mmHg to its new volume at standard atmosphere .

(18.0 mmHg) (77.0 L) = (760.0 mmHg) (x)

11: When the pressure on a gas increases, will the quantity increase or decrease?

Volume will decrease.

12: If the pressure on a gas is decreased by one-half, how large will the quantity change be?

It will double in size.

13: A gas occupies 4.31 litres at a pressure of 0.755 atm. Determine the quantity if the pressure is increased to 1.25 atm.

(0.755 atm) (4.31 litres) = (1.25 atm) (x)

14: 600.0 mL of a gas is at a pressure of 8.00 atm. What’s the quantity of the gas at 2.00 atm?

(8.00 atm) (600.0 mL) = (2.00 atm) (x)

15: 400.0 mL of a gas is under a pressure of 800.0 torr. What would the quantity of the gas be at a pressure of 1000.0 torr?

(800.0 torr) (400.0 mL) = (1000.0 torr) (x)

Conclusion

The laws are often expressed as an equation in many different ways. PV = k, where P denotes pressure, V denotes volume, and k denotes a constant. When the temperature is kept constant, the rule also can be used to determine the pressure or volume of a system.