4 g of hydrogen react with 9.023 × 1023 molecules of chlorine to form HCl gas. The total pressure after the reaction was found to be 700 mm. The partial pressure of HCl will be

Question

4 g of hydrogen react with 9.023 × 1023 molecules of chlorine to form HCl gas. The total pressure after the reaction was found to be 700 mm. The partial pressure of HCl will be (A) 3900 mm (B) 600 mm (C) 700 mm (D) 350 mm

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/528150eba33d66b8129325588a675099-.png" /> 3 / 2 mol of Cl 2 will react with 3 / 2 mol of H 2 to give(3/2) × 2=3.0 mol of HCl. So the total number of moles in the reaction =(2-(3/2))+0+3=3.5 Partial pressure of HCl =(3 × 700/3.5)=600 mm

Q. $4 g$ of hydrogen react with $9.023 \times 1 0^{23}$ molecules of chlorine to form $H Cl$ gas. The total pressure after the reaction was found to be $700 mm$ . The partial pressure of $H Cl$ will be

3900 mm

600 mm

700 mm

350 mm

$3/2$ mol of $C l_{2}$ will react with $3/2$ mol of $H_{2}$ to give $\frac{3}{2} \times 2 = 3.0 m o l$ of $H Cl$ . So the total number of moles in the reaction

$= (2 - \frac{3}{2}) + 0 + 3 = 3.5$

Partial pressure of $H Cl = \frac{3 \times 700}{3.5} = 600$ mm

Q. 4g of hydrogen react with 9.023×1023 molecules of chlorine to form HCl gas. The total pressure after the reaction was found to be 700mm. The partial pressure of HCl will be