Final answer:
To calculate the grams of gas in 5600 cm³ of chlorine gas at STP, use the ideal gas law equation to find the number of moles, then convert moles to grams using the molar mass of chlorine.
Step-by-step explanation:
To calculate the number of grams of gas present in 5600 cm³ of chlorine gas at STP, we need to use the ideal gas law equation: PV = nRT. At STP, the pressure (P) is 1 atm and the temperature (T) is 273 K. Since the gas is chlorine (Cl₂), the molar mass (M) is 70.906 g/mol. Rearranging the equation, we get n = PV/RT. Plugging in the values, we have n = (1 atm) * (5600 cm³) / (0.0821 L*atm/mol*K * 273 K). Calculating n, we find that it is equal to approximately 133.06 mol. Finally, we can convert mol to grams using the molar mass of chlorine: grams = (133.06 mol) * (70.906 g/mol). The final answer is approximately 9437.86 grams of chlorine gas.