Question

Statement : If equal masses of sodium metal and chlorine gas are allowed to react, some sodium will be leftover after all the chlorine is used up.
Statement 2 : The reaction required twice as many atoms of chlorine as sodium.

• A. Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.
• B. Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.
• C. Statement 1 is correct but Statement 2 is not correct.
• D. Statement 1 is not correct but Statement 2 is correct.
• E. Both the Statement 1 and Statement 2 are not correct.

Answer 1

Answer: (C)

Statement 1 is correct but Statement 2 is not correct.

$2Na+C{l}_2\to 2NaCl$

From the above reaction,

2 moles of $Na$ requires 1 mole of $C{l}_2$ to react completely

$\Rightarrow 2\times 23=46g$ of $Na$ requires $2\times 35.5=71g$ of $C{l}_2$ to react completely

Since the mass of sodium required for complete reaction is less than that of sodium, for same mass of sodium and chlorine, some sodium would be leftover as a result of incomplete reaction. Hence Statement 1 is correct

It can be clearly seen from the reaction that

Atoms of sodium =Atoms of chlorine=2

Hence Statement 2 is incorrect