$PCl_5 \rightleftharpoons PCl_3 + Cl_2 K_c = 1.844$
3.0 moles of $PCl_5$ is introduced in a 1 L closed reaction vessel at 380 K. The number of moles of $PCl_5$ at equilibrium is _________ $\times 10^{-3}$. (Round off to the Nearest Integer)
3.0 moles of $PCl_5$ is introduced in a 1 L closed reaction vessel at 380 K. The number of moles of $PCl_5$ at equilibrium is _________ $\times 10^{-3}$. (Round off to the Nearest Integer)
Show Hint
Correct Answer: 1258
Solution and Explanation
The equilibrium reaction is:
\[ \mathrm{PCl_5 \rightleftharpoons PCl_3 + Cl_2} \] Given: \[ K_c = 1.844 \] Volume of vessel = 1 L
Initial moles of $\mathrm{PCl_5}$ = 3.0
Since volume is 1 L, molarity equals number of moles.
Step 1: ICE table 
Step 2: Write equilibrium constant expression \[ K_c = \frac{[\mathrm{PCl_3}][\mathrm{Cl_2}]}{[\mathrm{PCl_5}]} \] \[ 1.844 = \frac{x^2}{3-x} \] Step 3: Solve the equation \[ 1.844(3-x) = x^2 \] \[ x^2 + 1.844x - 5.532 = 0 \] Solving using quadratic formula: \[ x = \frac{-1.844 + \sqrt{(1.844)^2 + 4(5.532)}}{2} \] \[ x \approx 1.74 \] Step 4: Moles of $\mathrm{PCl_5}$ at equilibrium \[ n_{\mathrm{PCl_5}} = 3.0 - x \] \[ = 3.0 - 1.74 = 1.26 \text{ mol} \] Step 5: Express in required format \[ 1.26 \text{ mol} = 1258 \times 10^{-3} \text{ mol (rounded)} \] \[ \boxed{1258} \]
Top JEE Main Chemistry Questions
What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)- At equilibrium the concentrations of and in a sealed vessel at . What will be for the reaction
- Find out the major products from the following reactions
Cobalt chloride when dissolved in water forms pink colored complex $X$ which has octahedral geometry. This solution on treating with cone $HCl$ forms deep blue complex, $\underline{Y}$ which has a $\underline{Z}$ geometry $X, Y$ and $Z$, respectively, are
- The correct order of atomic radii is:
Top JEE Main Law Of Chemical Equilibrium And Equilibrium Constant Questions
- $\text{The following concentrations were observed at 500 K for the formation of NH}_3 \text{ from N}_2 \text{ and H}_2\text{. At equilibrium: [N}_2] = 2 \times 10^{-2} \, \text{M, [H}_2] = 3 \times 10^{-2} \, \text{M, and [NH}_3] = 1.5 \times 10^{-2} \, \text{M. Equilibrium constant for the reaction is \_\_\_\_\_\_.}$
- The following reaction occurs in the Blast furnace where iron ore is reduced to iron metal:
\(\text{Fe}_2\text{O}_3(s) + 3\text{CO}(g) \rightleftharpoons 2\text{Fe}(l) + 3\text{CO}_2(g)\)
Using Le Chatelier's principle, predict which one of the following will not disturb the equilibrium. - The equilibrium $\mathrm{Cr_2O_7^{2-}} \rightleftharpoons 2\mathrm{CrO_4^{2-}}$ is shifted to the right in:
- For the given hypothetical reactions, the equilibrium constants are as follows:
\[ X \rightleftharpoons Y; \, K_1 = 1.0 \]
\[ Y \rightleftharpoons Z; \, K_2 = 2.0 \]
\[ Z \rightleftharpoons W; \, K_3 = 4.0 \]
The equilibrium constant for the reaction
\[ X \rightleftharpoons W\]
is: At \(-20^\circ \text{C}\) and 1 atm pressure, a cylinder is filled with an equal number of \(H_2\), \(I_2\), and \(HI\) molecules for the reaction:
\[H_2(g) + I_2(g) \rightleftharpoons 2HI(g)\] The \(K_P\) for the process is \(x \times 10^{-1}\).
(x = ___________)
Given: \(R = 0.082 \, \text{L atm K}^{-1} \text{mol}^{-1}\)
Top JEE Main Questions
- In a hydrogen like atom, when an electron jumps from the $M$ - shell to the $L$ - shell, the wavelength of emitted radiation is $\lambda$. If an electron jumps from $N$-shell to the $L$-shell, the wavelength of emitted radiation will be :
- Two masses $m$ and $\frac{m}{2}$ are connected at the two ends of a massless rigid rod of length $l$. The rod is suspended by a thin wire of torsional constant $k$ at the centre of mass of the rod-mass system(see figure). Because of torsional constant $k$, the restoring torque is $\tau =k\theta$ for angular displacement $\theta$. If the rod is rota ted by $\theta_0$ and released, the tension in it when it passes through its mean position will be:
What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)- The value of is
- The number of terms of an is even. The sum of the odd terms is and of the even terms is . The last term exceeds the first by . Then the number of terms in the series is ______.