How many moles of H2 (g) are there if Ph2 is 0.565 atm, volume is 50.4 mL, and temperature is 20.9 degrees Celsius?

Answer 1

To calculate the number of moles of H2 (g), 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/(mol·K))
T = temperature in Kelvin

First, we need to convert the given values to the appropriate units:

Pressure (Ph2) = 0.565 atm
Volume (V) = 50.4 mL = 0.0504 L
Temperature (T) = 20.9 degrees Celsius = 20.9 + 273.15 = 294.05 K

Now, we can plug these values into the ideal gas law equation:

0.565 atm * 0.0504 L = n * 0.0821 L·atm/(mol·K) * 294.05 K

0.028452 L·atm = n * 24.1338 L·atm/(mol·K)

Dividing by 24.1338 L·atm/(mol·K):

n = 0.028452 L·atm / 24.1338 L·atm/(mol·K)

n = 0.001179 mol

Therefore, there are approximately 0.001179 moles of H2 (g) present.