need help with #4 please don’t understand it really **Chemistry Worksheet: Reaction Calculations**1. **How many moles of $ \text{Li} $ and $ \text{H}_2 $ are yielded by the complete reaction of 2.24 moles of $ \text{Li} $ with excess water?** - Stoichiometry calculation: - $ 2 \, \text{mol} \, \text{Li} = 1 \, \text{mol} \, \text{H}_2 $ - $ 2.24 \, \text{moles} \, \text{Li} = 2.24 \div 2 = 1.12 \, \text{mol} \, \text{H}_2 $2. **Urea, $ (\text{NH}_2)_2\text{CO} $, is prepared by reacting ammonia with carbon dioxide as shown by:** \[ 2 \, \text{NH}_3 + \text{CO}_2 \rightarrow (\text{NH}_2)_2\text{CO} + \text{H}_2\text{O} \] - In one process, 927 g of $ \text{NH}_3 $ are treated with 1255 g of $ \text{CO}_2 $. - Calculate how many grams of $ (\text{NH}_2)_2\text{CO} $ are produced. **Calculations:** - Mass of $ \text{NH}_3 = 927 \, \text{g} $ - Mass of $ \text{CO}_2 = 1255 \, \text{g} $ - Mols of $ \text{NH}_3 $ and $ \text{CO}_2 $ based on molar masses and reactions used to determine reactant and product quantity.3. **The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000°C and is used in welding metals.** \[ 2 \, \text{Al} + \text{Fe}_2\text{O}_3 \rightarrow \text{Al}_2\text{O}_3 + 2 \, \text{Fe} \] - Calculate the mass of \( \text{Al}_2\text

First calculate the number of moles of calcium nitride. Use that moles to calculate the mass of…

4. The reaction between solid calcium nitride and water produces ammonia and calcium hydroxide. Ca3N2+ 6 H₂O2 NH3 + 3 Ca(OH)2 What mass of calcium hydroxide can be formed from the reaction when 34.25 g of calcium nitride react with excess water? a. b. If 47.02 g of calcium hydroxide was obtained from the reaction in (a), what is the percent yield of the reaction?

4. The reaction between solid calcium nitride and water produces ammonia and calcium hydroxide. Ca3N2+ 6 H₂O2 NH3 + 3 Ca(OH)2 What mass of calcium hydroxide can be formed from the reaction when 34.25 g of calcium nitride react with excess water? a. b. If 47.02 g of calcium hydroxide was obtained from the reaction in (a), what is the percent yield of the reaction?

Chemistry for Engineering Students

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Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

need help with #4 please don’t understand it really

**Chemistry Worksheet: Reaction Calculations**

1. **How many moles of $ \text{Li} $ and $ \text{H}_2 $ are yielded by the complete reaction of 2.24 moles of $ \text{Li} $ with excess water?**
- Stoichiometry calculation:
- $ 2 \, \text{mol} \, \text{Li} = 1 \, \text{mol} \, \text{H}_2 $
- $ 2.24 \, \text{moles} \, \text{Li} = 2.24 \div 2 = 1.12 \, \text{mol} \, \text{H}_2 $

2. **Urea, $ (\text{NH}_2)_2\text{CO} $, is prepared by reacting ammonia with carbon dioxide as shown by:**

\[
2 \, \text{NH}_3 + \text{CO}_2 \rightarrow (\text{NH}_2)_2\text{CO} + \text{H}_2\text{O}
\]

- In one process, 927 g of $ \text{NH}_3 $ are treated with 1255 g of $ \text{CO}_2 $.
- Calculate how many grams of $ (\text{NH}_2)_2\text{CO} $ are produced.

**Calculations:**
- Mass of $ \text{NH}_3 = 927 \, \text{g} $
- Mass of $ \text{CO}_2 = 1255 \, \text{g} $
- Mols of $ \text{NH}_3 $ and $ \text{CO}_2 $ based on molar masses and reactions used to determine reactant and product quantity.

3. **The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000°C and is used in welding metals.**

\[
2 \, \text{Al} + \text{Fe}_2\text{O}_3 \rightarrow \text{Al}_2\text{O}_3 + 2 \, \text{Fe}
\]

- Calculate the mass of \( \text{Al}_2\text

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