Question

How much sulfur must be burnt to achieve a mass of `150*g` with respect to `"sulfur dioxide"`?

Answer 1

This clearly should be in the chemistry section........I get approx. `50*g` `"sulfur"`.

Explanation:

And you will have to qualify what you mean by a table chart.

For all such reactions, we must first write a stoichiometrically balanced equation with respect to mass and charge......

Elemental sulfur can be burnt in air to give `SO_2(g)`, according to the following equation.......

`S(s) + O_2(g) rarr SO_2(g)`........if I was being pedantic I could write.....

`1/8S_8(s) + O_2(g) rarr SO_2(g)` but clearly the former equation reflects the stoichiometry faithfully.

We want `100*g` `SO_2(g)`, this represents a molar quantity of....

`(100.0*g)/((32.06+2xx16.00)*g*mol^-1)=1.56*mol`.

Given the 1:1 stoichiometry I must burn a `1.56*mol` quantity of elemental sulfur to get `1.56*mol` quantity of `SO_2(g)`....

i.e. a mass of `....1.56*cancel(mol)xx32.06*g*cancel(mol^-1)=50.0*g`