In the reaction 2 c o2 → 2 co, how many moles of carbon are needed to produce 66.0 g of carbon monoxide

mol e= mass / molar mass
mole of 2CO = 66.0g / (12.011 15.999)g / mol
mole of 2CO = 2.36 (CO and C has a 1:1 mole ratio)

mole of 2CO = 2.36 -> mole of 1 CO = 2.36 / 2 = 1.18

We got 2 moles of C, thus 1.18 x 2 = 2.36

So, we 2.36 moles of carbon are needed to produce 66.0 g of carbon monoxide in the reaction 2 C + O2 → 2 CO. To add, Carbon nonmetallic and tetravalent, thus, making four electrons available to form covalent chemical bonds.

nikitarahangdaleVT nikitarahangdaleVT · Answer 2 · 2022-04-07T14:35:42+02:00

In the given reaction moles of carbon are needed to produce 66.0 g of carbon monoxide is 2.35 moles.

How we calculate moles?

Moles of any substance will be calculated as:

n = W/M, where

W = given mass

M = molar mass

Given chemical reaction is:

2C + O₂ → 2CO

Moles of 66g of CO = 66g / 28g/mol = 2.35 mol

2 moles of CO = produced by 2 moles of carbon

2.35 moles of CO = produced by 2.35 moles of carbon

Hence, required moles of carbon are 2.35 moles.

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https://brainly.com/question/15374113