Calculate the number of moles and molecules of chlorine in 4.48\ dm^3 of chlorine at STP.

Correct answer: A. The number of mol of chlorine = 0.2 and number of molecules = 1.2044 × 10^ 23 . Volume of chlorine gas at STP = 4.48\ dm^3 Molar volume of an ideal gas at STP = 22.4\ dm^3mol^ -1 Number of moles of chlorine = Volume at STP Molar volume = (4.48)/(22.4) = 0.2\ mol Number of molecules of chlorine = Number of moles × N_A Number of molecules = 0.2 × 6.022 × 10^ 23 = 1.2044 × 10^ 23 Answer: The number of mol of chlorine = 0.2 and number of molecules = 1.2044 × 10^ 23 .

MHT CET 202624 AprilEvening Shift

Exam: MHT CET
Year: 2026
Date: 24 April
Shift: Evening Shift
Subject: Chemistry
Chapter: Some Basic Concepts of Chemistry

MHT CET 2026 · 24 April · Evening Shift · Chemistry · Some Basic Concepts of Chemistry

Calculate the number of moles and molecules of chlorine in 4.48\...

Calculate the number of moles and molecules of chlorine in

4.48\ \text{dm}^3

of chlorine at STP.

Options

AThe number of mol of chlorine $= 0.2$ and number of molecules $= 1.2044 \times 10^{23}$ .
BThe number of mol of chlorine $= 0.4$ and number of molecules $= 2.4088 \times 10^{23}$ .
CThe number of mol of chlorine $= 0.5$ and number of molecules $= 3.011 \times 10^{23}$ .
DThe number of mol of chlorine $= 0.6$ and number of molecules $= 3.6132 \times 10^{23}$ .

Correct answer

A. The number of mol of chlorine $= 0.2$ and number of molecules $= 1.2044 \times 10^{23}$ .

Step-by-step solution

Volume of chlorine gas at STP

= 4.48\ \text{dm}^3

Molar volume of an ideal gas at STP

= 22.4\ \text{dm}^3\text{mol}^{-1}

Number of moles of chlorine

= \dfrac{\text{Volume at STP}}{\text{Molar volume}} = \dfrac{4.48}{22.4} = 0.2\ \text{mol}

Number of molecules of chlorine

= \text{Number of moles} \times N_A

Number of molecules

= 0.2 \times 6.022 \times 10^{23} = 1.2044 \times 10^{23}

Answer: The number of mol of chlorine

= 0.2

and number of molecules

= 1.2044 \times 10^{23}

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