4g of $C O_{2}$ and 2.27 litre of $H_{2}$ at STP (273.15 K and 1 atm pressure) are mixed in a container. The total number of molecules present in the container will be:

6.022 \times 10^{25}

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6.022 \times 10^{23}

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6.022 \times 10^{22}

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12.044 \times 10^{22}

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Solution

The correct option is D $12.044 \times 10^{22}$
$1 m o l C O_{2} = 44 g$
$∴ 4.4 g$ of $C O_{2} = 0.1 m o l$
$\Rightarrow 1 m o l H_{2} = 22.4 l i t r e s$
$2.27 l i t e r s = 0.101 m o l$
$\Rightarrow$ Total number of moles $= 0.1 + 0.101 = 0.201 m o l$
Total number of molecules $= 0.201 \times 6.023 \times 10^{23}$
$= 1.21 \times 10^{23}$ molecules
$= 12.1 \times 10^{22}$ molecules
Hence, the answer is $12.1 \times 10^{22}$ molecules.

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One mole of any substance contains $6.022 \times 10^{23}$ atoms/molecules. Number of molecules of $H_{2} S O_{4}$ present in 100 mL of $0.02 M H_{2} S O_{4}$ solution is.............

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4g of CO2 and 2.27 litre of H2 at STP (273.15 K and 1 atm pressure) are mixed in a container. The total number of molecules present in the container will be:

The correct option is D 12.044×10221molCO2=44g∴4.4g of CO2=0.1mol⇒1molH2=22.4litres 2.27liters=0.101mol⇒ Total number of moles =0.1+0.101=0.201mol Total number of molecules =0.201×6.023×1023 =1.21×1023 molecules =12.1×1022 moleculesHence, the answer is 12.1×1022 molecules.

4g of $C O_{2}$ and 2.27 litre of $H_{2}$ at STP (273.15 K and 1 atm pressure) are mixed in a container. The total number of molecules present in the container will be: