If in an experimental reaction 32.5 mL were collected of hydrogen gas at 23.5 degrees celsius and 745.2 Torr what would be the volume corrected to STP conditions?
(P1V1/T1) = (P2V2/T2)
To find the volume of a gas at STP (Standard Temperature and Pressure), we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in this case, in Torr)
V = volume (we want to find this)
n = moles of gas
R = gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, we need to convert the given temperature from Celsius to Kelvin. The Kelvin temperature scale starts at absolute zero (-273.15°C), so to convert from Celsius to Kelvin, we add 273.15.
Given temperature = 23.5°C
Temperature in Kelvin = 23.5 + 273.15 = 296.65 K
Next, we convert the pressure from Torr to atm. The conversion factor is 1 atm = 760 Torr.
Given pressure = 745.2 Torr
Pressure in atm = 745.2 / 760 = 0.9795 atm
Now, we need to calculate the number of moles of hydrogen gas. To do this, we need to know the molar mass of hydrogen, which is 2.016 g/mol.
Assuming the hydrogen gas is at standard atomic weight (since you didn't mention otherwise), the molar mass of hydrogen is approximately 1.0079 g/mol.
Given volume = 32.5 mL
Convert volume to liters = 32.5 mL / 1000 mL/L = 0.0325 L
Now we can rearrange the ideal gas law equation to solve for the unknown volume:
V = nRT / P
To find n (moles of gas), we can use the formula:
n = mass / molar mass
Given that hydrogen has a molar mass of approximately 1.0079 g/mol, and assuming standard atomic weight, we can calculate the mass of hydrogen:
mass of hydrogen = n × molar mass
Since we don't have the mass information, we can't calculate the number of moles of hydrogen, which means we cannot find the volume at STP conditions.