0.016L
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Assuming Cl2 is in its gaseous form at standard temperature and pressure (STP), the volume would be 11.2 liters. This is calculated using the ideal gas law equation: V = (m/M) * (RT/P), where m is the mass of the gas, M is the molar mass of the gas, R is the ideal gas constant, T is the temperature, and P is the pressure.
For 2HCl(g) ==> H2(g) + Cl2(g) the Keq = [H2][Cl2]/[HCl]^2
You can use the ideal gas law to solve this problem. First, convert 0.30 g of Cl2 to moles. Then use the molar volume of gas at STP (22.4 L/mol) to determine the volume of Cl2 gas needed. Convert this volume to milliliters (1 L = 1000 mL) to find the answer.
The volume of the object can be calculated using the formula: volume = mass / density. Plugging in the values (mass = 25 g, density = 0.45 g/ml), the volume would be 55.56 ml.
The density of the object is 20 g/cm^3. Density is calculated by dividing the mass of the object by its volume. In this case, 500g ÷ 25cm^3 = 20 g/cm^3.
The density of Cl2 gas at standard temperature and pressure (STP) is approximately 3.214 g/L.