Therefore, the pressure of the 6.2 g of hydrogen gas in the 35 L container at 25°C is approximately 8.03 atm.
Step-by-step explanation:
The molar mass of hydrogen (H2) is 2.02 g/mol. So, for 6.2 g of hydrogen gas, the number of moles is: n = 6.2 g / 2.02 g/mol = 3.07 mol.
Next, we need to convert the temperature from Celsius to Kelvin since the Ideal Gas Law requires temperature in Kelvin. The conversion formula is: K = °C + 273.15.
Given that the temperature is 25°C, the temperature in Kelvin is: K = 25°C + 273.15 = 298.15 K.
Now we can substitute the values into the Ideal Gas Law equation. Rearranging the equation to solve for pressure (P), we have: P = (nRT) / V.
Plugging in the values: P = (3.07 mol)(0.0821 L·atm/mol·K)(298.15 K) / 35 L.
Simplifying the calculation: P = 8.03 atm