C(s)+o2(> co2(g) how many grams of carbon should be burned in an excess of oxygen at stp to obtain 2.21 l of carbon dioxide? 1.18 g 2.21 g 4.12 g 4.34 g

The correct answer is 1.18 g.

Explanation:

We are given a chemical equation:

We know that at STP conditions:

22.4L of volume is occupied by 1 mole of a gas.

So, 2.21L of carbon dioxide is occupied by = of carbon dioxide gas.

By Stoichiometry of the above reaction:

1 mole of carbon dioxide gas is produced by 1 mole of carbon

So, 0.0986 moles of carbon dioxide is produced by = of carbon.

Now, to calculate the mass of carbon, we use the equation:

Moles of carbon = 0.0986 mol

Molar mass of carbon = 12 g/mol

Putting values in above equation, we get:

Hence, the correct answer is 1.18 g.

step-by-step explanation:

whole numbers, zero or greater