Question

Formic acid, HCHO2, burns in oxygen to form carbon dioxide and water as follows:
HCHO2 (aq) + O2 (g) → 2 CO2 (g) + 2 H2O (l).
If a 3.15-g sample of formic acid was burned in 2.0 L of oxygen, what volume of carbon dioxide
would be produced? (Assume the reaction occurs at standard temperature and pressure, STP.)

Answer 1

Answer:

1.53216L

Explanation:

volume of o2 =2L

the reaction takes place @ stp

so by pv=nrt

n can be found

at stp 1atm , 273k , 0.0821 =r

1×2=n×273×0.0821

2=22.4n

n=2/22.4=1/11.2moles = 0.089mol

HCHO2 is methanoic acid

2HCHO2+O2==>2CO2+2H2O

molar mass of HCHO2 is 46.0254 g/mol

so in 3.15g methanoic acid

3.15÷46.0254 =0.0684 moles

moles of O2=0.089mol

moles oF HCHO2=0.0684 mol

in the reaction

moles of O2 = 1 mol

moles of HCHO2=2mol

now look for the limiting reactant

limiting reagent calculation , final answer calculation in the picture