How many litres of liquid CCl4 (Density= 1.5g/cm^3 ) must be measured out to contain 1 * 10^25 Cl atoms?

Here's what I did- 
No. of atoms of Cl - 10^25
No. of molecules of CCl₄ - 1/4 \* 10^25 or 25 \* 10^23


No. of moles = No . of particles/ Avogadro's No.
So (n) = 25\*10^23/6.02(approx) \*10^23
 (n) = 4.1
Also, No. of moles = Vol of gas at NTP/ 22.4 liters
so 4.1 = x/22.4 ======= x= 91.84 litres


But the answer in my textbook is .426 liters. What am I doing wrong?




The question asks for how many litres of **LIQUID** $\ce{CCl4}$. Note what you have done is for **GAS**. So the steps would be:


1. Find the amount of substance of $\ce{CCl4}$ required.
2. Multiply it with its molecular weight (154 g/mol).
3. Use its density to find the volume.


Hope you understood your mistake.


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