130cm3 of a gas excarts a pressure 750mmhg . calculate it pressure if its volume is increase to 150cm3 at 35oc
constant Temp?
P1*V1=P2*V2
P2= P1*V1/V2
ANSWER MY QUESTION
To calculate the new pressure of the gas when its volume increases to 150 cm^3 at 35°C, we can use the combined gas law, which states:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure (what we need to calculate)
V2 = final volume
T2 = final temperature
Given:
P1 = 750 mmHg
V1 = 130 cm^3
T1 = unknown
P2 = unknown
V2 = 150 cm^3
T2 = 35°C
To begin, we need to convert the temperature T2 from Celsius to Kelvin since the gas law requires temperature in Kelvin.
T2(K) = T2(°C) + 273.15
T2(K) = 35 + 273.15
T2(K) = 308.15 K
Now we can substitute the given values into the combined gas law equation:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
By rearranging the equation, we can solve for P2:
P2 = (P1 * V1 * T2) / (V2 * T1)
To find T1, we can use the ideal gas law:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles (which is constant)
R = ideal gas constant (also constant)
T = temperature
Rearranging this equation gives:
T = (P * V) / (n * R)
Since the ideal gas law does not specify units for pressure and volume, we can use any consistent units. In this case, we'll use atm for pressure and liters for volume.
Converting the given values:
P1 = 750 mmHg * (1 atm / 760 mmHg) ≈ 0.987 atm
V1 = 130 cm^3 * (1 L / 1000 cm^3) ≈ 0.13 L
T1 = (P1 * V1) / (n * R)
Substituting these values into the combined gas law:
P2 = (P1 * V1 * T2) / (V2 * T1)