What volume of H2 gas, in mL, would be occupied by 0.00465 moles of H2 gas at a temperature of 0 °C and a pressure of 760 mmHg?
V = nRT/P
you'll have to look up R (the gas comstant), T = 273 in Kelvin, and P must be converted to Pascals (unless you can find a gas constant in mmHg)
To determine the volume of H2 gas, we can use the Ideal Gas Law, which states:
PV = nRT
Where:
P is the pressure,
V is the volume,
n is the number of moles,
R is the ideal gas constant (0.0821 L·atm/(mol·K) or 62.36 mmHg·mL/(mol·K)),
T is the temperature in Kelvin.
First, let's convert the given temperature from 0 °C to Kelvin:
0 °C + 273.15 = 273.15 K
Now we can plug in the given values into the ideal gas law equation:
PV = nRT
P = 760 mmHg
V = ?
n = 0.00465 moles
R = 62.36 mmHg·mL/(mol·K)
T = 273.15 K
Rearranging the equation to solve for V, we have:
V = (nRT) / P
Substituting the values:
V = (0.00465 moles * 62.36 mmHg·mL/(mol·K) * 273.15 K) / 760 mmHg
Calculating this expression will give us the volume of H2 gas in mL.