Answer: There are 8.26 mol of hydrogen present in the 17 liter container.
Explanation: PV = nRTwhere P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is the temperature.
Substituting the given values, we have:(3.23 atm) x (0.346 L) = (0.34 mol) x (R) x TR, the gas constant, is 0.08206 L atm/mol K.
Simplifying the equation and solving for T, we get:T = (3.23 atm x 0.346 L) / (0.34 mol x 0.08206 L atm/mol K) = 107 K
Converting to Celsius, we get:T = 107 K - 273.15 = -166.15°C
Therefore, the temperature is approximately -166.15°C.
To find the amount of hydrogen present in a 17 liter container at a pressure of 446 torr and 80.9°C, we can use the Ideal Gas Law equation again.PV = nRTwhere P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
First, we need to convert the pressure to atm and the volume to L:446 torr = 0.587 atm17 L = 17000 mL
Next, we can solve for n:n = (PV) / (RT)where R is still the gas constant, and T is the temperature in Kelvin.
Converting the temperature to Kelvin:80.9°C + 273.15 = 354.05 K
Substituting the given values, we have:n = (0.587 atm x 17000 mL) / (0.08206 L atm/mol K x 354.05 K)
Simplifying and solving for n, we get:n = 8.26 mol. Therefore, there are 8.26 mol of hydrogen present in the 17 liter container.