Question

How many litres of chlorine gas, C1,, can be obtained at
40°C and 1.03 atm from 9.41 g of hydrogen chloride, according
to the following equation?
2KMnO,(s) + 16HCl(aq) →
81,0 (1)+2KCl(aq) + 2MnCl2 (aq) + 5C12, (g)​

Answer 1

Answer:

2.02 litres of chlorine gas can be obtained at 40°C and 1.03 atm from 9.41 g of hydrogen chloride

Explanation:

Given mass of HCl = 9.41 g.

Number of moles of HCl = given mass / molar mass of HCl.

                                         = 9.41 g / (36.46  g/mol)

                                         = 0.26 moles

According to the balanced chemical equation:

16 moles of HCl → 5 moles of $Cl_{2}$

0.26 moles of HCl → 5*0.26/16 moles of $Cl_{2}$

                                 = 0.081 moles of $Cl_{2}$

According to ideal gas equation,

PV = nRT

P- pressure

V- volume

n- number of moles

R - gas constant= 0.082 L atm/K/mol

T - temperature in kelvin=273+40 = 313 K

V = nRT/P

   = 0.081 * 0.082 * 313 / 1.03

    = 2.02 litres of $Cl_{2}$