Question 8 of 30 The reaction of hydrogen with nitrogen to produce ammonia is shown below. If there are 6 moles of nitrogen, how many moles of hydrogen are needed to react completely with the nitrogen? N2(g) + 3H2(g) → 2NH3(g) O A. 6 О В. 2 Ос. 18 O D. 3 SUBMIT

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Chapter1: Chemical Foundations
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**Pretest: Unit 5**

**Question 8 of 30**

The reaction of hydrogen with nitrogen to produce ammonia is shown below. If there are 6 moles of nitrogen, how many moles of hydrogen are needed to react completely with the nitrogen?

\[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \]

*Options:*

- **A. 6**
- **B. 2**
- **C. 18**
- **D. 3**

*Graph/Diagram Explanation:*

There is no graph or detailed diagram provided in this question. The visual only contains a chemical equation describing the reaction between nitrogen gas (\(\text{N}_2\)) and hydrogen gas (\(\text{H}_2\)) to produce ammonia (\(\text{NH}_3\)), along with multiple-choice answers to select the correct number of moles needed in the reaction based on the provided chemical equation. The focus is on stoichiometry calculations.

\[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \]

The given options (A, B, C, D) require understanding the mole ratio between nitrogen and hydrogen from the balanced chemical equation.
Transcribed Image Text:**Pretest: Unit 5** **Question 8 of 30** The reaction of hydrogen with nitrogen to produce ammonia is shown below. If there are 6 moles of nitrogen, how many moles of hydrogen are needed to react completely with the nitrogen? \[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \] *Options:* - **A. 6** - **B. 2** - **C. 18** - **D. 3** *Graph/Diagram Explanation:* There is no graph or detailed diagram provided in this question. The visual only contains a chemical equation describing the reaction between nitrogen gas (\(\text{N}_2\)) and hydrogen gas (\(\text{H}_2\)) to produce ammonia (\(\text{NH}_3\)), along with multiple-choice answers to select the correct number of moles needed in the reaction based on the provided chemical equation. The focus is on stoichiometry calculations. \[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \] The given options (A, B, C, D) require understanding the mole ratio between nitrogen and hydrogen from the balanced chemical equation.
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