Question

12kg of carbon burns fully in 64g of pure oxygen amd the volume of products is measured at 273k and 1 atm the volume of gas is

Answer 1

Given,

Mass of carbon =$12 kg$

Moles of Carbon=$\dfrac{12}{12}=1000\text{mol}$

Mass of Oxygen =64g

Moles of oxygen =$\dfrac{64}{32}=2\text{mol}$

The Balance Chemical reaction is given by-

$C+O_2\rightarrow CO_2$

Here The limiting reagent is $O_2$ ,

Thus, Mole of $CO_2$ = Mole of $O_2=2\text{mol}$

Also, Pressure $P=1 \text{atm}$

Temprature, $T=273K$

Universal gas constant, $R=8.314Jk^-mol^-$

Let Volume be V

According to ideal gas equation,

$PV=nRT$

$1\times V=2\times 8.314\times273$

$V=4539.44ml=4.54l$

Hence Volume of product formed is $4.54l$