Q2. Ammonia gas and hydrogen chloride gas combine to make ammonium chloride. STP? (3
volume of ammonia at STP is needed to react with 47.7 liters of hydrogen chloride at STP?
marks)
Q3. How many grams of sodium do you have to put into water to make 30 liters of
hydrogen at STP? (3 marks)
Q4. copper + sulfuric acid copper II sulfate + water + sulfur dioxide
How many moles of copper are needed to produce 1000 L of SO2? (3 marks)
mor

Question

Q2. Ammonia gas and hydrogen chloride gas combine to make ammonium chloride. STP? (3
volume of ammonia at STP is needed to react with 47.7 liters of hydrogen chloride at STP?
marks)
Q3. How many grams of sodium do you have to put into water to make 30 liters of
hydrogen at STP? (3 marks)
Q4. copper + sulfuric acid

copper II sulfate + water + sulfur dioxide
How many moles of copper are needed to produce 1000 L of SO2? (3 marks)
mor

UpStudy AI · Accepted Answer

**Q2**

The reaction between ammonia and hydrogen chloride is

$$
\text{NH}_3\,(g) + \text{HCl}\,(g) \rightarrow \text{NH}_4\text{Cl}\,(s)
$$

Since the reactants combine in a 1:1 mole ratio and at STP equal volumes correspond to equal moles, the volume of ammonia required is the same as the volume of hydrogen chloride. Therefore, for 47.7 L of hydrogen chloride gas, you need

$$
47.7\text{ L of NH}_3
$$

---

**Q3**

The reaction between sodium and water is

$$
2\text{Na} + 2\text{H}_2\text{O} \rightarrow 2\text{NaOH} + \text{H}_2
$$

At STP, one mole of any ideal gas occupies $$22.4$$ L. Therefore, the number of moles of hydrogen gas in $$30$$ L is

$$
n_{\text{H}_2} = \frac{30\text{ L}}{22.4\text{ L/mol}} \approx 1.339\text{ mol}
$$

From the reaction, $$2$$ moles of sodium produce $$1$$ mole of hydrogen. Thus, the moles of sodium required are

$$
n_{\text{Na}} = 2 \times n_{\text{H}_2} \approx 2 \times 1.339 \approx 2.678\text{ mol}
$$

The molar mass of sodium is approximately $$23$$ g/mol, so the mass of sodium needed is

$$
\text{Mass of Na} = 2.678\text{ mol} \times 23\text{ g/mol} \approx 61.6\text{ g}
$$

---

**Q4**

The reaction between copper and sulfuric acid is

$$
\text{Cu} + 2\text{H}_2\text{SO}_4 \rightarrow \text{CuSO}_4 + \text{SO}_2 + 2\text{H}_2\text{O}
$$

Here, the stoichiometry shows that $$1$$ mole of copper produces $$1$$ mole of sulfur dioxide ($$\text{SO}_2$$). At STP, one mole of gas occupies $$22.4$$ L. The number of moles of $$\text{SO}_2$$ produced from $$1000$$ L is

$$
n_{\text{SO}_2} = \frac{1000\text{ L}}{22.4\text{ L/mol}} \approx 44.6\text{ mol}
$$

Thus, the moles of copper needed are

$$
n_{\text{Cu}} \approx 44.6\text{ mol}
$$
**Q2** To react with 47.7 liters of hydrogen chloride at STP, you need **47.7 liters of ammonia**. --- **Q3** To produce 30 liters of hydrogen gas at STP, you need approximately **61.6 grams of sodium**. --- **Q4** To produce 1000 liters of sulfur dioxide at STP, you need **44.6 moles of copper**.

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