We have to prepare 500 gr of a HCl solution 15% by mass:
H2SO4 + NaCl at a Temperature of 100°C
NAHSO4 is also produced
The equation is:
H2SO4 + NaCl->NaHSO4 + HCl
1) How many grams of H2SO4 93% by mass and of NaCl do we need if we consider a loss of 3,O% of HCl during the preparation?
2) Find the total volume of HCl (gaz) produced during this preparation if the temperature is 15°C and the pression is 750mm Hg?
Thank you very much for the help
To solve the given problem, we need to follow the following steps:
1) Calculate the amount of H2SO4 (93% by mass) and NaCl required to prepare the HCl solution.
To find the mass of H2SO4 needed:
Given: Mass of HCl solution = 500 g
Percentage of H2SO4 in the solution = 93%
Loss of HCl during preparation = 3%
Since H2SO4 and HCl have a 1:1 mole ratio, the molar mass of H2SO4 (98.09 g/mol) is used as a conversion factor.
The equation is: H2SO4 + NaCl -> NaHSO4 + HCl
From the balanced equation, 1 mole of H2SO4 produces 1 mole of HCl.
Mass of H2SO4 needed (in grams) = Mass of HCl solution * Percentage of H2SO4 / (100% - Loss of HCl)
Mass of H2SO4 needed = 500 g * 93% / (100% - 3%)
Mass of H2SO4 needed = 500 g * 0.93 / 0.97
Mass of H2SO4 needed = 482.47 g
To find the mass of NaCl needed:
From the balanced equation, 1 mole of NaCl produces 1 mole of HCl.
The molar mass of NaCl (58.44 g/mol) is used as a conversion factor.
Mass of NaCl needed (in grams) = Mass of HCl solution * (Percentage of H2SO4 / (100% - Loss of HCl)) * (Molar mass of NaCl / Molar mass of H2SO4)
Mass of NaCl needed = 500 g * (93% / (100% - 3%)) * (58.44 g/mol / 98.09 g/mol)
Mass of NaCl needed = 500 g * (0.93 / 0.97) * (58.44 g/mol / 98.09 g/mol)
Mass of NaCl needed = 284.35 g
Therefore, we need 482.47 grams of H2SO4 (93% by mass) and 284.35 grams of NaCl.
2) Calculate the total volume of HCl (gas) produced at 15°C and a pressure of 750 mmHg.
To find the volume of HCl, we need to use the Ideal Gas Law equation:
PV = nRT
Given:
Temperature (T) = 15°C = 15 + 273.15 K (convert to Kelvin)
Pressure (P) = 750 mmHg = 750/760 atm (convert to atm)
The ideal gas constant (R) = 0.0821 L·atm/mol·K
To find the moles of HCl gas:
From the balanced equation, 1 mole of H2SO4 produces 1 mole of HCl.
Moles of HCl = Moles of H2SO4 = Mass of H2SO4 / Molar mass of H2SO4
Moles of HCl = 482.47 g / 98.09 g/mol
Moles of HCl = 4.92 mol
Using the ideal gas law:
PV = nRT
V = (nRT) / P
V = (4.92 mol * 0.0821 L·atm/mol·K * (15 + 273.15) K) / (750/760 atm)
V = (4.92 * 0.0821 * 288.15) / (750/760) L
V = 1.92 L
Therefore, the total volume of HCl gas produced at 15°C and a pressure of 750 mmHg is 1.92 liters.