Question

The value of x is ________.
 

Answer 1

Correct Answer: 3.57

Step 1: Reaction of Sn with HCl
The reaction between tin (Sn) and hydrochloric acid (HCl) produces tin(II) chloride (SnCl₂):
\( \text{Sn} + \text{2HCl} \rightarrow \text{SnCl}_2 + \text{H}_2 \)
Thus, 1 mole of Sn produces 1 mole of SnCl₂.

Step 2: Moles of ammonium salt produced
The organic salt produced is an ammonium salt. From the problem, we know that the moles of the organic salt are calculated using the formula:
\[ \text{Moles of ammonium salt} = \frac{\text{mass of organic salt}}{\text{molar mass of organic salt}} \] The mass of the organic salt produced is given as 1.29 g, and its molar mass is \( 129 \, \text{g/mol} \) (molar mass of ammonium salt).
So, the moles of ammonium salt are:
\[ \frac{1.29}{129} = 0.01 \, \text{mol} \]

Step 3: Moles of nitrobenzene used
The moles of nitrobenzene are equal to the moles of ammonium salt produced (since the reaction is quantitative).
Thus, the moles of nitrobenzene used are 0.01 mol.
\[ \text{Moles of nitrobenzene} = 0.01 \, \text{mol} \]

Step 4: Number of equivalents of nitrobenzene and SnCl₂
The number of equivalents of nitrobenzene is equal to the number of equivalents of SnCl₂. The equivalent of nitrobenzene is 6 times the moles of nitrobenzene (since the reaction involves 6 equivalents of nitrobenzene for every 1 equivalent of SnCl₂):
\[ \text{No. of equivalents of nitrobenzene} = 6 \times 0.01 = 0.06 \, \text{equivalents} \] Since the number of equivalents of SnCl₂ is equal to the number of equivalents of nitrobenzene, the number of equivalents of SnCl₂ is 0.06.
Now, the number of moles of SnCl₂ can be found by dividing the equivalents by 2 (since each mole of SnCl₂ has 2 equivalents):
\[ \text{Moles of SnCl}_2 = \frac{0.06}{2} = 0.03 \, \text{mol} \]

Step 5: Calculate the mass of Sn
Now, we know that 1 mole of Sn reacts to form 1 mole of SnCl₂. So, the moles of Sn required are equal to the moles of SnCl₂, which is 0.03 mol.
Now, the mass of Sn required can be calculated using the molar mass of Sn (119 g/mol):
\[ \text{Mass of Sn} = 0.03 \, \text{mol} \times 119 \, \text{g/mol} = 3.57 \, \text{g} \]

Final Answer:
The value of \( x \), the mass of Sn required, is \( 3.57 \, \text{g} \).

Answer 2

Step 1: Reaction between Sn and HCl
The reaction between Sn and HCl is as follows:
\( \text{Sn} + 2HCl \rightarrow \text{SnCl}_2 + H_2 \).
This reaction produces tin(II) chloride (SnCl₂).

Step 2: Moles of ammonium salt produced
The organic salt produced is formed from the reaction of SnCl₂ with nitrobenzene in the presence of HCl.
The given mass of the organic salt is 1.29 g.
The molar mass of the organic salt is given as 129 g/mol.
To find the moles of ammonium salt, use the formula:
\(\text{Moles of organic salt} = \frac{\text{mass}}{\text{molar mass}} = \frac{1.29}{129} = 0.01 \, \text{mol}\).

Step 3: Moles of nitrobenzene required
From the stoichiometry of the reaction, the moles of nitrobenzene are equal to the moles of organic salt formed.
Thus, the moles of nitrobenzene required are 0.01 mol.
Now, to find the mass of nitrobenzene (y), use the formula:
\( \text{Mass of nitrobenzene} = \text{moles} \times \text{molar mass of nitrobenzene} \).
The molar mass of nitrobenzene is given as 123 g/mol.
Therefore, the mass of nitrobenzene (y) is:
\( y = 0.01 \times 123 = 1.23 \, \text{g} \).

Final Answer:
The value of y is 1.23 g.