The reaction, `2C+O_(2)rarr2CO` is carried out by taking `24` g of carbon and `96` g `O_(2)`, find out :
(a) Which reactant is left in excess ?
(b) How much of it is left ?
(c) How many mole of `CO` are formed ?
(d) How many `g` of other reactant should be taken so that nothing is left at the end of reaction ?

Explanation

To solve the problem step by step, we will analyze the reaction \(2C + O_2 \rightarrow 2CO\) with the given amounts of carbon and oxygen.

### Step 1: Calculate the moles of each reactant.
1. **Molar mass of Carbon (C)** = 12 g/mol
- Given mass of Carbon = 24 g
- Moles of Carbon = \(\frac{24 \text{ g}}{12 \text{ g/mol}} = 2 \text{ moles}\)

2. **Molar mass of Oxygen (O2)** = 32 g/mol (since O has a molar mass of 16 g/mol, and O2 has two O atoms)
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