If 4 moles of gas are added to a container that already holds 1 mole of gas, how will the pressure change inside the container?
PV = nRT
Since n is increased, what must happen to P.
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To determine how the pressure will change inside the container when 4 moles of gas are added to a container that already holds 1 mole of gas, we can use the ideal gas law. The ideal gas law equation is formulated as:
PV = nRT
Where:
P represents the pressure of the gas
V represents the volume of the container
n represents the number of moles of gas
R is the ideal gas constant
T represents the temperature in Kelvin
Given that the volume and temperature of the container are constant, we can simplify the equation to:
P1 / n1 = P2 / n2
Where:
P1 is the initial pressure
n1 is the initial number of moles
P2 is the final pressure (after adding 4 moles)
n2 is the final number of moles (1 + 4 = 5 moles in this case)
Now, to find how the pressure will change, we can substitute the known values into the equation:
P1 / 1 = P2 / 5
To solve for P2, we can rearrange the equation:
P2 = P1 * (n2 / n1)
P2 = P1 * (5 / 1)
P2 = 5 * P1
This calculation shows that the final pressure, P2, will be 5 times the initial pressure, P1.
Therefore, when 4 moles of gas are added to a container that already holds 1 mole of gas, the pressure inside the container will increase by a factor of 5.