Atomic masses: C 12, F 19, Cl 35.5; Avogadro constant N_A = 6.02x10^23 mol^-1. Assume each molecule of CF2Cl2 in 24.2 g of the compound loses exactly one Cl atom by photolysis. How many Cl atoms are released, in units of 10^23? Give the answer to two decimals.

JEE Main levelNumerical answerDifficulty 2 of 3ev088

Atomic masses: C 12, F 19, Cl 35.5; Avogadro constant $N_{A} = 6.02 \times 1 0^{23} mo l^{- 1}$ . Assume each molecule of $CF X_{2} Cl X_{2}$ in $24.2 g$ of the compound loses exactly one Cl atom by photolysis. How many Cl atoms are released, in units of $1 0^{23}$ ? Give the answer to two decimals.

Numerical answer type, tolerance 0.01.

Molar mass of

CF X_{2} Cl X_{2}

12 + 2 (19) + 2 (35.5) = 121 g mo l^{- 1}

. Moles =

24.2/121 = 0.200

. Number of Cl atoms =

0.200 \times 6.02 \times 1 0^{23} = 1.204 \times 1 0^{23}

, i.e. 1.20 in units of

1 0^{23}