How many grams of HCl are required to produce 11.2 L of Cl2.The reaction occurs in the presence of excess HCl and at STP

Explanation:

Equation of reaction:

2HCl → H₂ + Cl₂

From the equation of reaction,

From ideal gas equation,

PV = nRT

P = pressure of the ideal gas

V = volume of the gas

n = number of moles

R = ideal gas constant

T = temperature of the gas

At STP,

P = 1.0atm

T = 273.15K

R = 0.082J/mol.K

PV = nRT

1 .0 × 11.2 = n × 0.082 × 273.15

11.2 = 22.398n

n = 11.2 / 22.398

n = 0.50mole

From the equation of reaction,

2 moles of HCl = 1 mole of Cl₂

X moles HCl = 0.5mole

X = (2 × 0.5) / 1

X = 1 mole of HCL

Number of mole = mass / molar mass

Molar mass of HCl = 1 + 35.5 = 36.5g/mol

Mass = number of mole × molar mass

Mass = 1 × 36.5

Mass = 36.5g

36.5g of HCl is required to to produce 11.2L of Cl₂

i believe it is 40–40–20%

explanation:

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)