A 2.0 L sample at 20°C and 750 torr contains 0.5moles of a gas. If 0.1 mole of the gas at the same temperature and pressure is added to the sample, what is the new volume of the gass show your solution
We can use the Ideal Gas Law, PV = nRT, to solve for the new volume.
The Ideal Gas Law states that the product of pressure (P), volume (V), and the number of moles (n) of a gas is equal to the product of the gas constant (R) and the temperature (T) in Kelvin.
Answers & Comments
Answer:
the new volume of the gas is 2.16 L.
Explanation:
We can use the Ideal Gas Law, PV = nRT, to solve for the new volume.
The Ideal Gas Law states that the product of pressure (P), volume (V), and the number of moles (n) of a gas is equal to the product of the gas constant (R) and the temperature (T) in Kelvin.
So, we can rearrange the equation to solve for V:
V = (nRT) / P
Given that the initial conditions are:
n = 0.5 moles
T = 20°C = 293 K
P = 750 torr
R = 0.0821 L·atm/mol·K
We can calculate the initial volume as:
V = (0.5 moles) * (0.0821 L·atm/mol·K) * (293 K) / (750 torr)
V = 2.0 L
Now, we can use the same equation to find the new volume after 0.1 moles are added to the sample:
V = (0.5 moles + 0.1 moles) * (0.0821 L·atm/mol·K) * (293 K) / (750 torr)
V = 2.16 L
So, the new volume of the gas is 2.16 L.