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Q. No.Why \(NH_4Cl\) is added before \(NH_4OH\) for the ppt. of \(Fe^{3+}\) ions?
1. To decrease \(OH^-\) ion concentration
2. To increase \(Cl^-\)ion concentration
3. To increase \(NH^+_4\) ion concentration
4. To decrease \(H^+\) ion concentration
Subtopic: Common Ion Effect |
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Level 3: 35%-60%
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Consider the following equilibrium reaction:
\(\mathrm{H}_2+\mathrm{I}_2 \rightleftharpoons 2 \mathrm{HI}\)
At equilibrium, if the number of molecules of \(\mathrm{H}_2,~ \mathrm{I}_2,\) and \(\mathrm{HI}\) are equal, and the equilibrium constant \(\mathrm{K}_{\mathrm{p}}=\mathrm{t} \times 10^{-1}\), the value of t is:
\(\mathrm{H}_2+\mathrm{I}_2 \rightleftharpoons 2 \mathrm{HI}\)
At equilibrium, if the number of molecules of \(\mathrm{H}_2,~ \mathrm{I}_2,\) and \(\mathrm{HI}\) are equal, and the equilibrium constant \(\mathrm{K}_{\mathrm{p}}=\mathrm{t} \times 10^{-1}\), the value of t is:
| 1. | 10.0 | 2. | 0.01 |
| 3. | 0.10 | 4. | 1.0 |
Subtopic: Kp, Kc & Factors Affecting them |
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Level 2: 60%+
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Consider the following reaction at equilibrium at a temperature of T Kelvin, with a given equilibrium constant \(K_c=3 \times 10^{-13}:\)
\(\mathrm{SO}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_3(\mathrm{~g})\)
Now, consider the reverse reaction:
\(2 \mathrm{SO}_3(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})\)
The equilibrium constant for this reaction is denoted as \(K_{c^{\prime}}^{\prime}\) which can be expressed as \(a \times 10^{+b}\) in scientific notation.
What is the value of \(a+b\) ?
1. 26
2. 29
3. 20
4. 19
\(\mathrm{SO}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_3(\mathrm{~g})\)
Now, consider the reverse reaction:
\(2 \mathrm{SO}_3(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})\)
The equilibrium constant for this reaction is denoted as \(K_{c^{\prime}}^{\prime}\) which can be expressed as \(a \times 10^{+b}\) in scientific notation.
What is the value of \(a+b\) ?
1. 26
2. 29
3. 20
4. 19
Subtopic: Kp, Kc & Factors Affecting them |
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In the following reaction, HCl formed is titrated with 0.2 moles of NaOH.
Calculate the mass of \(\mathrm{C}_2 \mathrm{H}_5\mathrm{NH}_2\) taken initially:
\(\mathrm{C}_2 \mathrm{H}_5\mathrm{NH}_2+\mathrm{NaNO}_2 \xrightarrow{\mathrm{HCl}} \mathrm{A} \xrightarrow{\mathrm{H}_2 \mathrm{O}} \mathrm{HCl}+\text { Alcohol }+\mathrm{N}_2\)
1. 4
2. 6
3. 9
4. 8
Calculate the mass of \(\mathrm{C}_2 \mathrm{H}_5\mathrm{NH}_2\) taken initially:
\(\mathrm{C}_2 \mathrm{H}_5\mathrm{NH}_2+\mathrm{NaNO}_2 \xrightarrow{\mathrm{HCl}} \mathrm{A} \xrightarrow{\mathrm{H}_2 \mathrm{O}} \mathrm{HCl}+\text { Alcohol }+\mathrm{N}_2\)
1. 4
2. 6
3. 9
4. 8
Subtopic: Salt Hydrolysis & Titration |
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Level 2: 60%+
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Hints
Consider the following equilibrium reaction:
\(\mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s})+3 \mathrm{CO}(\mathrm{g}) \rightleftharpoons 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_2(\mathrm{~g})~\)
Which of the following will not affect the equilibrium state?
(I) Addition of \(\mathrm{Fe}_2 \mathrm{O}_3\)
(II) Addition of \(CO_2\)
(III) Decreasing the mass of \(\mathrm{Fe}_2 \mathrm{O}_3\)
(IV) Removal of \(CO\)
1. (II) and (IV)
2. (I) and (IV)
3. (I) and (III)
4. All will affect the equilibrium state
\(\mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s})+3 \mathrm{CO}(\mathrm{g}) \rightleftharpoons 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_2(\mathrm{~g})~\)
Which of the following will not affect the equilibrium state?
(I) Addition of \(\mathrm{Fe}_2 \mathrm{O}_3\)
(II) Addition of \(CO_2\)
(III) Decreasing the mass of \(\mathrm{Fe}_2 \mathrm{O}_3\)
(IV) Removal of \(CO\)
1. (II) and (IV)
2. (I) and (IV)
3. (I) and (III)
4. All will affect the equilibrium state
Subtopic: Le Chatelier's principle |
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Level 2: 60%+
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Find relation between \(\mathrm{K_P}\) and \(\mathrm{K_C}\) for this given reaction:
\(\mathrm{C}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}(\mathrm{g})\)
1. \(K_P=K_C(R T)^1 \)
2. \( K_P=K_C(R T)^{-1}\)
3. \(K_P=K_C(R T)^{1 / 2} \)
4. \( K_P=K_C(R T)^{-1 / 2}\)
\(\mathrm{C}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}(\mathrm{g})\)
1. \(K_P=K_C(R T)^1 \)
2. \( K_P=K_C(R T)^{-1}\)
3. \(K_P=K_C(R T)^{1 / 2} \)
4. \( K_P=K_C(R T)^{-1 / 2}\)
Subtopic: Kp, Kc & Factors Affecting them |
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Level 1: 80%+
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Consider the following equilibrium reactions along with their respective equilibrium constants:
\(\begin{aligned} & x \rightleftharpoons y~ ;~~ k_1=1 \\ & y \rightleftharpoons z ~; ~~k_2=2 \\ & z \rightleftharpoons w~ ; ~~k_3=4 \end{aligned}\)
Now, calculate the overall equilibrium constant \(k_{\text{eq}}\) for the reaction:
\( \mathrm{x} \rightleftharpoons \mathrm{w}\)
Choose the correct answer:
\(\begin{aligned} & x \rightleftharpoons y~ ;~~ k_1=1 \\ & y \rightleftharpoons z ~; ~~k_2=2 \\ & z \rightleftharpoons w~ ; ~~k_3=4 \end{aligned}\)
Now, calculate the overall equilibrium constant \(k_{\text{eq}}\) for the reaction:
\( \mathrm{x} \rightleftharpoons \mathrm{w}\)
Choose the correct answer:
| 1. | 10 | 2. | 8 |
| 3. | 2 | 4. | 4 |
Subtopic: Kp, Kc & Factors Affecting them |
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Consider the given reaction:
\(\mathrm{Cr}_2 \mathrm{O}_7^{2-} \rightleftharpoons \mathrm{CrO}_4^{2-}\)
In which medium does the reaction proceed in the forward direction?
1. Acidic medium
2. Basic medium
3. Neutral medium
4. Slightly acidic medium
\(\mathrm{Cr}_2 \mathrm{O}_7^{2-} \rightleftharpoons \mathrm{CrO}_4^{2-}\)
In which medium does the reaction proceed in the forward direction?
1. Acidic medium
2. Basic medium
3. Neutral medium
4. Slightly acidic medium
Subtopic: Le Chatelier's principle |
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Level 3: 35%-60%
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\(\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g})+\dfrac{1}{2} \mathrm{C}(\mathrm{g}) \)
In the above reaction, the correct relation among \( \text{K}_p\), \( \alpha\) and equilibrium pressure (p) is:
1. \(\mathrm{K}_{\mathrm{p}}=\dfrac{\alpha^{1 / 2} 2 \mathrm{p}^{1 / 2}}{(2+\alpha)^{1 / 2}}\)
2. \(K_p=\dfrac{\alpha^{1 / 2} p^{3 / 2}}{(2+\alpha)^{3 / 2}}\)
3. \(\mathrm{K}_{\mathrm{p}}=\dfrac{\alpha^{1 / 2} 2 \mathrm{p}^{1 / 2}}{(2+\alpha)^{3 / 2}}\)
4. \(\mathrm{K}_{\mathrm{p}}=\dfrac{\alpha^{3 / 2} \mathrm{p}^{1 / 2}}{(2+\alpha)^{1 / 2}(1-\alpha)}\)
Subtopic: Kp, Kc & Factors Affecting them |
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Consider the following reaction, the expression for \(\text{K}_c\) is :
\([\mathrm{Fe}(\mathrm{SCN})]_{(\mathrm{aq})}^{2+} \rightleftharpoons{\mathrm{Fe}^{3+}_{\mathrm{(aq)}}}+ {\mathrm{SCN}^{-}_\mathrm{(aq)}}\)
1. \(\mathrm{K}_{\mathrm{c}}=\dfrac{\left[\mathrm{Fe}^{3+}\right]\left[\mathrm{SCN}^{-}\right]}{\left[[\mathrm{Fe}(\mathrm{SCN})]^{2+}\right]}\)
2. \(\mathrm{K}_{\mathrm{c}}=\dfrac{\left[\mathrm{Fe}^{3+}\right]^2\left[\mathrm{SCN}^{-}\right]}{\left[[\mathrm{Fe}(\mathrm{SCN})]^{2+}\right]}\)
3. \(\mathrm{K}_{\mathrm{c}}=\dfrac{\left[\mathrm{Fe}^{3+}\right]^2\left[\mathrm{SCN}^{-}\right]^2}{\left[[\mathrm{Fe}(\mathrm{SCN})]^{2+}\right]}\)
4. \(\mathrm{K}_{\mathrm{c}}=\dfrac{\left[\mathrm{Fe}^{3+}\right]^3\left[\mathrm{SCN}^{-}\right]}{\left[[\mathrm{Fe}(\mathrm{SCN})]^{2+}\right]}\)
\([\mathrm{Fe}(\mathrm{SCN})]_{(\mathrm{aq})}^{2+} \rightleftharpoons{\mathrm{Fe}^{3+}_{\mathrm{(aq)}}}+ {\mathrm{SCN}^{-}_\mathrm{(aq)}}\)
1. \(\mathrm{K}_{\mathrm{c}}=\dfrac{\left[\mathrm{Fe}^{3+}\right]\left[\mathrm{SCN}^{-}\right]}{\left[[\mathrm{Fe}(\mathrm{SCN})]^{2+}\right]}\)
2. \(\mathrm{K}_{\mathrm{c}}=\dfrac{\left[\mathrm{Fe}^{3+}\right]^2\left[\mathrm{SCN}^{-}\right]}{\left[[\mathrm{Fe}(\mathrm{SCN})]^{2+}\right]}\)
3. \(\mathrm{K}_{\mathrm{c}}=\dfrac{\left[\mathrm{Fe}^{3+}\right]^2\left[\mathrm{SCN}^{-}\right]^2}{\left[[\mathrm{Fe}(\mathrm{SCN})]^{2+}\right]}\)
4. \(\mathrm{K}_{\mathrm{c}}=\dfrac{\left[\mathrm{Fe}^{3+}\right]^3\left[\mathrm{SCN}^{-}\right]}{\left[[\mathrm{Fe}(\mathrm{SCN})]^{2+}\right]}\)
Subtopic: Kp, Kc & Factors Affecting them |
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