LiOH reacts with `CO_(2)` form `Li_(2)CO_(3)` (atomic mass of Li= 7). The amount of `CO_(2)` (in g) consumed by 1g of LiOH is closest to.

Options

A. 0.916
B. 1.832
C. 0.544
D. 1.088

Explanation

To solve the problem of how much CO₂ is consumed by 1 g of LiOH, we can follow these steps:

### Step 1: Write the balanced chemical equation
The reaction between lithium hydroxide (LiOH) and carbon dioxide (CO₂) can be represented by the following balanced equation:

\[ 2 \text{LiOH} + \text{CO}_2 \rightarrow \text{Li}_2\text{CO}_3 + \text{H}_2\text{O} \]

### Step 2: Calculate the molar mass of LiOH
The molar mass of LiOH can be calculated as follows:
- Atomic mass of Lithium (Li) = 7 g/mol
- Atomic mass of Oxygen (O) = 16 g/mol
- Atomic mass of Hydrogen (H) = 1 g/mol

Thus, the molar mass of LiOH is:
\[ \text{Molar mass of LiOH} = 7 + 16 + 1 = 24 \text{ g/mol} \]

### Step 3: Calculate the number of moles of LiOH in 1 g
To find the number of moles of LiOH in 1 g, we use the formula:
\[ \text{Number of moles} = \frac{\text{mass}}{\text{molar mass}} \]

Substituting the values:
\[ \text{Number of moles of LiOH} = \frac{1 \text{ g}}{24 \text{ g/mol}} = 0.04167 \text{ mol} \]

### Step 4: Use the stoichiometry of the reaction
From the balanced equation, we see that 2 moles of LiOH react with 1 mole of CO₂. Therefore, the moles of CO₂ required for the moles of LiOH can be calculated as follows:
\[ \text{Moles of CO}_2 = \frac{0.04167 \text{ mol LiOH}}{2} = 0.02083 \text{ mol CO}_2 \]

### Step 5: Calculate the mass of CO₂ consumed
Next, we need to calculate the mass of CO₂ consumed. The molar mass of CO₂ is:
- Atomic mass of Carbon (C) = 12 g/mol
- Atomic mass of Oxygen (O) = 16 g/mol (and there are 2 O atoms)

Thus, the molar mass of CO₂ is:
\[ \text{Molar mass of CO}_2 = 12 + (2 \times 16) = 44 \text{ g/mol} \]

Now, we can find the mass of CO₂ consumed:
\[ \text{Mass of CO}_2 = \text{Number of moles} \times \text{Molar mass} \]
\[ \text{Mass of CO}_2 = 0.02083 \text{ mol} \times 44 \text{ g/mol} = 0.916 \text{ g} \]

### Step 6: Round to the nearest whole number
The question asks for the amount of CO₂ consumed in grams, which is closest to:
\[ \approx 0.92 \text{ g} \]

Thus, the final answer is approximately **0.92 g** of CO₂ consumed by 1 g of LiOH.