Question

CS2(l) + O2(g) CO2(g) + SO2(g)
Consider the above unbalanced equation. What mass of CS2 is required to react with excess oxygen to produce 985 mL of SO2 at 465 mm Hg and 54.0°C? Use molar masses with at least as many significant figures as the data given.

Answer 1

Answer:

Given,

325g of Na2O2 is reacted with water

Molar mass of Na2O2=78g/mol

∴ Number of moles of Na2O2 given=78g/mol325g

=4.166 moles

The reaction involved is

2Na2O2+2H2O⟶4NaOH+O2

2 moles of Na2O2 gives 1 moles of O2

∴4.166 moles of Na2O2 gives ⟶24.166 moles of O2

=2.083 moles of O2

Now,

The molar mass of CS2=76/gmol

The reaction involved id 

CS2+3O2⟶CO2+2SO2

1 mole of CS2 requires 3 moles of 

Answer 2

Explanation:

Given,

325g of Na

2

O

2

is reacted with water

Molar mass of Na

2

O

2

=78g/mol

∴ Number of moles of Na

2

O

2

given=

78g/mol

325g

=4.166 moles

The reaction involved is

2Na

2

O

2

+2H

2

O⟶4NaOH+O

2

2 moles of Na

2

O

2

gives 1 moles of O

2

∴4.166 moles of Na

2

O

2

gives ⟶

2

4.166

moles of O

2

=2.083 moles of O

2

Now,

The molar mass of CS

2

=76/gmol

The reaction involved id

CS

2

+3O

2

⟶CO

2

+2SO

2

1 mole of CS

2

requires 3 moles of O

2

Now, 2.083 moles of O

2

will react with x moles of CS

2

to produce SO

2

& CO

2

x=0.6943 moles of CS

2

∴ The mass of CS

2

which can be completely oxidized by 2.083 moles of O

2

=0.6943mol×76g/mol

=52.76g