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Calculate the number of atoms of hydrogen present in 5.6 g of urea, [tex]$\left( NH _2\right)_2 CO$[/tex]. Also, calculate the number of atoms of [tex]$N$[/tex], [tex]$C$[/tex], and [tex]$O$[/tex].

(Ans.: No. of atoms of [tex]$H = 2.24 \times 10^{23}$[/tex], [tex]$N = 1.124 \times 10^{23}$[/tex], [tex]$C = 0.562 \times 10^{23}$[/tex], [tex]$O = 0.562 \times 10^{23}$[/tex])

Calculate the mass of sulfur dioxide produced by burning 16 g of sulfur in excess of oxygen in the contact process.

(Average atomic mass: [tex]$S = 32$[/tex])



Answer :

GinnyAnswer
Sure, let's work through the problem step by step.

### Step 1: Understanding the chemical reaction
The chemical reaction for burning sulfur in excess oxygen is:
[tex]\[ S + O_2 \rightarrow SO_2 \][/tex]

This means one mole of sulfur ([tex]\(S\)[/tex]) reacts with one mole of oxygen ([tex]\(O_2\)[/tex]) to form one mole of sulfur dioxide ([tex]\(SO_2\)[/tex]).

### Step 2: Given data
- Mass of sulfur ([tex]\(m_{\text{S}}\)[/tex]): 16 grams
- Molar mass of sulfur ([tex]\(M_{\text{S}}\)[/tex]): 32 grams per mole
- Molar mass of sulfur dioxide ([tex]\(M_{\text{SO}_2}\)[/tex]): 64 grams per mole

### Step 3: Calculate moles of sulfur
To find the moles of sulfur, use the formula:
[tex]\[ \text{Moles of sulfur} = \frac{\text{Mass of sulfur}}{\text{Molar mass of sulfur}} \][/tex]
Substitute the given values:
[tex]\[ \text{Moles of sulfur} = \frac{16 \text{ grams}}{32 \text{ grams/mole}} = 0.5 \text{ moles} \][/tex]

### Step 4: Determine moles of sulfur dioxide produced
From the balanced chemical equation, we see that one mole of sulfur produces one mole of sulfur dioxide. Therefore, 0.5 moles of sulfur will produce 0.5 moles of sulfur dioxide.

### Step 5: Calculate the mass of sulfur dioxide produced
To find the mass of sulfur dioxide produced, use the formula:
[tex]\[ \text{Mass of } SO_2 = \text{Moles of } SO_2 \times \text{Molar mass of } SO_2 \][/tex]
Substitute the calculated moles and given molar mass:
[tex]\[ \text{Mass of } SO_2 = 0.5 \text{ moles} \times 64 \text{ grams/mole} = 32 \text{ grams} \][/tex]

### Final answer:
The mass of sulfur dioxide produced by burning 16 grams of sulfur in excess oxygen is 32 grams.

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