A gas occupied 870 ml under a pressure of 720 mmHg at a temperature of 17C ,the next day it was measured under a pressure 0f 750 mmHg at a temperature of 21C.what volume did the gas occupy under these condition
See your other post. Same formula.
To find the volume of the gas under the given conditions, we can use the combined gas law, which incorporates Boyle's law, Charles's law, and Gay-Lussac's law. The formula for the combined gas law is:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure
V2 = final volume (what we want to find)
T2 = final temperature
Let's plug in the given values:
P1 = 720 mmHg
V1 = 870 ml (which is equivalent to 0.87 L, as 1 L = 1000 ml)
T1 = 17°C (which needs to be converted to Kelvin by adding 273.15; thus, T1 = 17 + 273.15 = 290.15 K)
P2 = 750 mmHg
T2 = 21°C (which needs to be converted to Kelvin as well; thus, T2 = 21 + 273.15 = 294.15 K)
Now we can rearrange the formula to solve for V2:
V2 = (P1 * V1 * T2) / (P2 * T1)
V2 = (720 mmHg * 0.87 L * 294.15 K) / (750 mmHg * 290.15 K)
Now, let's convert the units to cancel out mmHg and calculate:
V2 = (720 * 0.87 * 294.15) / (750 * 290.15)
V2 = 227253.78 / 217613.62
V2 ≈ 1.044 L (rounded to three decimal places)
Therefore, under the new conditions, the gas occupies approximately 1.044 liters of volume.