Final answer:
To calculate the mass of HCl consumed during the reaction, we need to use the ideal gas law equation PV = nRT. After plugging in the given values and solving for the number of moles of chlorine gas, we can determine the mass of HCl consumed using the molar mass and the balanced chemical equation. The correct answer is not listed among the options provided.
Step-by-step explanation:
In order to calculate the mass of HCl consumed during the reaction, we need to use the ideal gas law equation:
PV = nRT
Where P is the pressure in atm, V is the volume in liters, n is the number of moles, R is the ideal gas constant (0.0821 L atm/mol K), and T is the temperature in Kelvin.
We can rearrange this equation to solve for n:
n = PV / RT
First, we need to convert the temperature from Celsius to Kelvin:
T = 28 + 273.15 = 301.15 K
Next, we need to convert the volume from milliliters to liters:
V = 750 / 1000 = 0.75 L
Using the given pressure, temperature, and volume, we can now calculate the number of moles of chlorine gas:
n = (788/760) * 0.75 / (0.0821 * 301.15) = 0.0262 moles
The molar mass of HCl is 36.461 g/mol. Since the balanced chemical equation for the reaction is 1 mole of Cl2 reacts to produce 2 moles of HCl, the mass of HCl consumed can be calculated as follows:
mass HCl = 0.0262 moles * (2 * 36.461 g/mol) = 1.90 g
Therefore, the correct answer is approximately 1.90 g, which is not listed among the options provided.