Question

The temperature of a gas filled in a vessel is 273 k and pressure is 1.60 * 10^-3 determine the number of molecules in unit volume of the vessel

Answer 1

Two moles of an ideal gas undergo a reversible isothermal expansion from 2.303l to 23.03l at 27 degree celsius . the change in entropy i.

Two moles of an ideal gas undergo a reversible isothermal expansion from 2.303l to 23.03l at 27 degree celsius . the change in entropy i

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Answer 2

The number of molecules in unit volume of the vessel according to the given conditions are $0.427 \times 10^{20}$ atoms.

Explanation:

The given data is as follows.

           T = 273 K,        P = $1.60 \times 10^{-3}$ atm

           V = 1.0 L,          n = ?

According to the ideal gas equation,

                        PV = nRT

Hence, putting the given values into the above formula as follows.

                    PV = nRT

    $1.60 \times 10^{-3} atm \times 1 L = n \times 0.0821 L atm/mol K \times 273 K$

                    n = $0.071 \times 10^{-3}$ mol

Also, we know that 1 mole of a substance contains $6.022 \times 10^{23}$ moles of atoms. Therefore, molecules contained by $0.071 \times 10^{-3}$ mol will be as follows.

            $0.071 \times 10^{-3} mol \times 6.022 \times 10^{23} atoms/mol$

             = $0.427 \times 10^{20}$ atoms

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