A sample of hydrogen gas (H2) has a volume 8.56L at a temperature of 0 degree and a pressure of 1.5atm. calculate the number of moles of H2 molecules present in this gas sample.
We can use the ideal gas law to solve this problem:
PV = nRT
where:
P = pressure = 1.5 atm
V = volume = 8.56 L
n = number of moles
R = gas constant = 0.08206 L atm/mol K
T = temperature = 273 K (0 degree Celsius)
Rearranging the equation to solve for n:
n = PV/RT
Plugging in the values:
n = (1.5 atm * 8.56 L) / (0.08206 L atm/mol K * 273 K)
n = 0.573 moles
Therefore, there are 0.573 moles of H2 molecules present in this gas sample.
To calculate the number of moles of H2 molecules present in the gas sample, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/K·mol)
T = temperature (in Kelvin)
First, let's convert the temperature from degrees Celsius to Kelvin:
0 degrees Celsius = 273.15 Kelvin
Now, let's plug in the values into the equation and solve for n:
(1.5 atm)(8.56 L) = n(0.0821 L·atm/K·mol)(273.15 K)
12.84 atm·L = n(22.414 L·atm/mol·K)
n = (12.84 atm·L) / (22.414 L·atm/mol·K)
n ≈ 0.574 moles
Therefore, approximately 0.574 moles of H2 molecules are present in this gas sample.