Question

which of the following has maximum number of molecules
1)2.7g of NH3 2)1ட so2 3)2ட of cl2 at stp 4)0.1 mol of H2S

Answer 1

Answer: 1) 2.7g of $NH_3$

Explanation:According to avogadro's law, 1 mole of every substance occupies 22.4 Liters at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

1) 2.7 g of $NH_3$

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}$

$\text{Number of moles}=\frac{2.7g}{17g/mol}=0.16moles$ (1L=1000ml)

Now 1 mole of $NH_3$ molecule contains = $6.023\times 10^{23}$ of molecules

0.16 mole of $NH_3$ molecule contains = $0.16\times 6.023\times 10^{23}=0.96\times 10^{23}$ molecules

2) 1L of $SO_2$

$\text{Number of moles}=\frac{\text{Given volume}}{\text {Molar Volume}}$

$\text{Number of moles}=\frac{1L}{22.4L}=0.04 moles$

Now 1 mole of $SO_2$ molecule contains = $6.023\times 10^{23}$ of molecules

0.04 mole of $NH_3$ molecule contains = $0.04\times 6.023\times 10^{23}=0.24\times 10^{23}$ molecules

3) 2L of $Cl_2$

$\text{Number of moles}=\frac{\text{Given volume}}{\text {Molar Volume}}$

$\text{Number of moles}=\frac{2L}{22.4L}=0.09moles$

Now 1 mole of $Cl_2$ molecule contains = $6.023\times 10^{23}$ of molecules

0.09 mole of $Cl_2$ molecule contains = $0.09\times 6.023\times 10^{23}=0.54\times 10^{23}$ molecules

4. 0.1 mol of $H_2S$

Now 1 mole of $H_2S$ molecule contains = $6.023\times 10^{23}$ of molecules

0.1 mole of $H_2S$ molecule contains = $0.1\times 6.023\times 10^{23}=0.6023\times 10^{23}$ molecules

Answer 2

Answer: The correct answer is Option 1.

Explanation:

According to mole concept:

1 mole of a compound contains $6.022\times 10^{23}$ number of molecules

For the given options:

• Option 1: 2.7 g of $NH_3$

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mas}}{\text{Molar mass}}$

Given mass of ammonia = 2.7 g

Molar mass of ammonia = 17 g/mol

Putting values in above equation, we get:

$\text{Moles of ammonia}=\frac{2.7g}{17g/mol}=0.16mol$

Using mole concept:

0.16 moles of ammonia gas will occupy = $0.16\times 6.022\times 10^{23}=9.6352\times 10^{22}$

Number of molecules in given amount of ammonia gas = $9.6352\times 10^{22}$

• Option 2: 1 L of $SO_2$ at STP

At STP conditions:

22.4 L of volume is occupied by 1 mole of a gas

So, 1 L of volume will be occupied by = $\frac{1}{22.4}\times 1=0.045mol$ of sulfur dioxide gas

Using mole concept:

0.045 moles of sulfur dioxide gas will occupy = $0.045\times 6.022\times 10^{23}=2.71\times 10^{22}$

Number of molecules in given amount of sulfur dioxide gas = $2.71\times 10^{22}$

• Option 3: 2 L of $Cl_2$ at STP

At STP conditions:

22.4 L of volume is occupied by 1 mole of a gas

So, 2 L of volume will be occupied by = $\frac{1}{22.4}\times 2=0.09mol$ of chlorine gas

Using mole concept:

0.09 moles of chlorine gas will occupy = $0.09\times 6.022\times 10^{23}=5.42\times 10^{22}$

Number of molecules in given amount of chlorine gas = $5.42\times 10^{22}$

• Option 4: 0.1 mol of $H_2S$

Using mole concept:

0.1 moles of hydrogen sulfide gas will occupy = $0.1\times 6.022\times 10^{23}=6.022\times 10^{22}$

Number of molecules in given amount of hydrogen sulfide = $6.022\times 10^{22}$

Hence, the correct answer is Option 1.