3.2 moles of hydrogen iodide was heated in a sealed bulb at 444°C till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be 22 %. The number of moles of hydrogen iodide present at equilibrium is

Question

3.2 moles of hydrogen iodide was heated in a sealed bulb at 444°C till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be 22 %. The number of moles of hydrogen iodide present at equilibrium is (A) 2.496 (B) 1.87 (C) 2 (D) 4

Tardigrade Admin · Accepted Answer

(22/100) × 3.2 =0.704 ∴ at equil. moles of HI = 3.2 - 0.704 = 2.496

Q. $3.2$ moles of hydrogen iodide was heated in a sealed bulb at $444° C$ till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be $22%$ . The number of moles of hydrogen iodide present at equilibrium is

$2.496$

$1.87$

$2$

$4$

$\frac{22}{100} \times 3.2 = 0.704$
$∴$ at equil. moles of $H I = 3.2 - 0.704 = 2.496$

Q. 3.2 moles of hydrogen iodide was heated in a sealed bulb at 444°C till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be 22%. The number of moles of hydrogen iodide present at equilibrium is

2.496

1.87

2

4

10022​×3.2=0.704 ∴ at equil. moles of HI=3.2−0.704=2.496

Q. $3.2$ moles of hydrogen iodide was heated in a sealed bulb at $444° C$ till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be $22%$ . The number of moles of hydrogen iodide present at equilibrium is

$2.496$

$1.87$

$2$

$4$

$\frac{22}{100} \times 3.2 = 0.704$
$∴$ at equil. moles of $H I = 3.2 - 0.704 = 2.496$