Answer :
Final answer:
Using the Ideal Gas Law and the given conditions, the mass of Cl2 in the 10.0L gas tank is found to be approximately 101 grams, corresponding to answer choice d.
Explanation:
To determine the mass of Cl2 in a 10.0L tank at 27°C (300K) and 3.50 atm pressure, we can use the Ideal Gas Law PV=nRT. First, we need to rearrange the formula to solve for n (the number of moles) as n = PV / (RT). We will use R = 0.0821 L·atm/(mol·K), the ideal gas constant.
Substituting the given values we get: n = (3.50 atm × 10.0 L) / (0.0821 L·atm/(mol·K) × 300 K) = 1.42 mol.
Now to find the mass of chlorine, we use the molar mass of Cl2, which is 70.90 g/mol (from 2 x 35.45 g for each Cl atom). The mass (m) is then m = n × molar mass = 1.42 mol × 70.90 g/mol = 100.678 grams.
Therefore, the mass of Cl2 contained in the tank is approximately 101 grams, which corresponds to answer choice d.
