Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid. hcl(aq), as described by the chemical equationmno2(s) + 4hcl(aq) --> mncl2(aq) + 2h2o(l) + cl2(g)how much mno2(s) should be added to excess hcl (aq) to obtain 235 ml of cl2(g) at 25 degrees c and 805 torr?

0.88 g

Explanation:

Using ideal gas equation to calculate the moles of chlorine gas produced as:-

where,

P = pressure of the gas = 805 Torr

V = Volume of the gas = 235 mL = 0.235 L

T = Temperature of the gas =

R = Gas constant =

n = number of moles of chlorine gas = ?

Putting values in above equation, we get:

According to the reaction:-

1 mole of chlorine gas is produced when 1 mole of manganese dioxide undergoes reaction.

So,

0.01017 mole of chlorine gas is produced when 0.01017 mole of manganese dioxide undergoes reaction.

Moles of = 0.01017 moles

Molar mass of = 86.93685 g/mol

So,

Applying values, we get that:-

0.88 g of should be added to excess HCl (aq) to obtain 235 mL of at 25 degrees C and 805 Torr.

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