At 16°C a sample of ammonia gas exerts a pressure of 11.7 atm. What is the pressure when the volume of the gas is reduced to one-fourth of the original value at the same temperature
so the inital Temp=16 C
initial Pressure. 11.7
final pressure-unknown
temperature-same
what next?
You omitted some of the problem.
initial T = 16 C
p = 11.7 atm
final pressure = ??, the unknown.
final T = 16 (apparently doesn't change).
initial volume = ?
final volume = 1/4 the original volume.
What I usually do is to assume a value for V1 (a convenient number of 4), that makes the final volume 1 (1/4 of 4 = 1).
Then use P1V1 = P2V2 and solve for P2.
okay thank you
With your information I did
p1v1=p2v2
(11.7)( 4)= P2(1)
my final answer 46.8 atm
To solve this problem, you can use Boyle's Law, which states that at constant temperature, the pressure and volume of a gas are inversely proportional.
1. First, convert the initial temperature from Celsius to Kelvin. Add 273 to the temperature value to get the Kelvin temperature. In this case, the initial temperature is 16°C, so the Kelvin temperature is 16 + 273 = 289 K.
2. Since the temperature remains constant, we can directly apply Boyle's Law. According to Boyle's Law, the product of the initial pressure and volume is equal to the product of the final pressure and final volume. Mathematically, it can be written as:
P1 * V1 = P2 * V2
Where:
P1 is the initial pressure (11.7 atm),
V1 is the initial volume,
P2 is the final pressure (unknown),
V2 is the final volume (one-fourth of the initial volume).
3. Since the final volume is reduced to one-fourth, we can write V2 = V1/4.
4. Substituting the known values into the equation, we have:
11.7 atm * V1 = P2 * (V1/4)
5. Simplify the equation:
V1 cancels out on both sides, giving us:
11.7 atm = P2/4
6. Multiply both sides of the equation by 4 to isolate P2:
4 * 11.7 atm = P2
7. Calculate the final pressure:
P2 = 46.8 atm
So, the final pressure when the volume is reduced to one-fourth of the original value at the same temperature is 46.8 atm.