Nitrogen dioxidegas and liquid water react to form aqueous nitric acid and nitrogen monoxidegas. Suppose you have 7mol NO2  and  11mol of H2) in a reactor.

What would be the limiting reactant? Enter its chemical formula below.

To find the limiting reactant, we need to first write the balanced chemical equation for the reaction between nitrogen dioxide (\(NO_2\)) and water (\(H_2O\)):

\[
3 NO_2 (g) + H_2O (l) \rightarrow 2 HNO_3 (aq) + NO (g)
\]

From the balanced equation, we can see that 3 moles of \(NO_2\) react with 1 mole of \(H_2O\) to form the products.

Now, we will compare the mole ratio of the reactants you have with the ratio required by the balanced equation:

- You have 7 moles of \(NO_2\).
- You have 11 moles of \(H_2O\).

### Step 1: Calculate the mole ratio based on the available moles
- According to the equation, 3 moles of \(NO_2\) react with 1 mole of \(H_2O\). So for 7 moles of \(NO_2\), the required moles of \(H_2O\) would be:

\[
\frac{7}{3} = 2.33 \text{ moles of } H_2O \text{ needed}.
\]

### Step 2: Compare with the available moles of \(H_2O\)
- You have 11 moles of \(H_2O\), which is much more than the required 2.33 moles.
  
Therefore, \(NO_2\) is the limiting reactant because you do not have enough of it to react with all the \(H_2O\).

### The limiting reactant is: 
**\(NO_2\)**

Would you like to go over the process in more detail, or do you have any questions?

Here are 5 related questions to expand your understanding:
1. How do you determine the excess reactant in a chemical reaction?
2. What is the concept of the limiting reactant in stoichiometry?
3. How do you calculate the theoretical yield of a product based on the limiting reactant?
4. Why is balancing a chemical equation important for stoichiometry problems?
5. What happens when a limiting reactant is completely consumed in a reaction?

**Tip**: Always double-check the mole ratio from the balanced equation before determining the limiting reactant.

Nitrogen dioxide gas and liquid water react to form aqueous nitric acid and nitrogen monoxide gas. Suppose you have 7 mol NO2 and 11 mol of H2O in a reactor. What would be the limiting reactant? Enter its chemical formula below.

Find out how to determine the limiting reactant in a chemical reaction between nitrogen dioxide (NO2) and water (H2O). This problem involves key stoichiometric concepts and mole ratio calculations. Ideal for high school chemistry students in grades 10-12.

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