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Chemical Equilibrium

229049 What is the equilibrium expression for the reaction,

1 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]^5}\)
2 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{5\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]}\)
3 \(\mathrm{K}_{\mathrm{c}}=\left[\mathrm{O}_2\right]^5\)
4 \(\mathrm{K}_{\mathrm{c}}=\frac{1}{\left[\mathrm{O}_2\right]^5}\)
JCECE - 2008
Chemical Equilibrium

229051 Which of the following statements is true when equilibrium is established in the reaction?
$A+B \quad C+D, K_{C}=10$

1 $[\mathrm{C}][\mathrm{D}]=[\mathrm{A}][\mathrm{B}]$
2 $[\mathrm{C}]=[\mathrm{A}]$ and $[\mathrm{B}]=[\mathrm{D}]$
3 $[\mathrm{A}][\mathrm{B}]=0.1[\mathrm{C}][\mathrm{D}]$
4 $[\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=[\mathrm{D}]=10 \mathrm{M}$
AP-EAPCET 24.08.2021 Shift-II
Chemical Equilibrium

229052 For a reaction taking place in three steps, the rate constants are $k_{1}, k_{2}$ and $k_{3}$ and overall rate constant is $k=\frac{k_{1} k_{3}}{k_{2}}$. If the energies of activation $E_{1}, E_{2}$ and $E_{3}$ are 60,30 and $10 \mathrm{~kJ}$ $\mathrm{mol}^{-1}$ respectively, then the overall energy of activation is

1 $30 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $40 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $60 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$
AMU-2014
Chemical Equilibrium

229055 $630 \mathrm{mg}$ of oxalic acid is equivalent to

1 $100 \mathrm{~mL}$ of $0.2 \mathrm{~N} \mathrm{KMnO}_{4}$
2 $100 \mathrm{~mL}$ of $0.05 \mathrm{~N} \mathrm{KMnO}_{4}$
3 $100 \mathrm{~mL}$ of $0.01 \mathrm{~N} \mathrm{KMnO}_{4}$
4 $100 \mathrm{~mL}$ of $0.1 \mathrm{~N} \mathrm{KMnO}_{4}$
COMEDK-2011
Chemical Equilibrium

229056 For the reaction $\mathrm{A}+3 \mathrm{~B} \longrightarrow 2 \mathrm{C}+\mathrm{D}$, which one of the following is not correct?

1 Rate of disappearance of $\mathrm{A}=$ Rate of formation of $\mathrm{D}$
2 Rate of formation of $\mathrm{C}=\frac{2}{3} \times$ Rate of disappearance of $\mathrm{B}$
3 Rate of formation of $\mathrm{D}=\frac{1}{3} \times$ Rate of disappearance of $\mathrm{B}$
4 Rate of disappearance of $\mathrm{A}=2 \times$ Rate of formation of $\mathrm{C}$
AP- EAMCET(Medical) -2010
NEET DIGITAL LIBRARY
Chemical Equilibrium

229049 What is the equilibrium expression for the reaction,

1 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]^5}\)
2 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{5\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]}\)
3 \(\mathrm{K}_{\mathrm{c}}=\left[\mathrm{O}_2\right]^5\)
4 \(\mathrm{K}_{\mathrm{c}}=\frac{1}{\left[\mathrm{O}_2\right]^5}\)
JCECE - 2008
Chemical Equilibrium

229051 Which of the following statements is true when equilibrium is established in the reaction?
$A+B \quad C+D, K_{C}=10$

1 $[\mathrm{C}][\mathrm{D}]=[\mathrm{A}][\mathrm{B}]$
2 $[\mathrm{C}]=[\mathrm{A}]$ and $[\mathrm{B}]=[\mathrm{D}]$
3 $[\mathrm{A}][\mathrm{B}]=0.1[\mathrm{C}][\mathrm{D}]$
4 $[\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=[\mathrm{D}]=10 \mathrm{M}$
AP-EAPCET 24.08.2021 Shift-II
Chemical Equilibrium

229052 For a reaction taking place in three steps, the rate constants are $k_{1}, k_{2}$ and $k_{3}$ and overall rate constant is $k=\frac{k_{1} k_{3}}{k_{2}}$. If the energies of activation $E_{1}, E_{2}$ and $E_{3}$ are 60,30 and $10 \mathrm{~kJ}$ $\mathrm{mol}^{-1}$ respectively, then the overall energy of activation is

1 $30 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $40 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $60 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$
AMU-2014
Chemical Equilibrium

229055 $630 \mathrm{mg}$ of oxalic acid is equivalent to

1 $100 \mathrm{~mL}$ of $0.2 \mathrm{~N} \mathrm{KMnO}_{4}$
2 $100 \mathrm{~mL}$ of $0.05 \mathrm{~N} \mathrm{KMnO}_{4}$
3 $100 \mathrm{~mL}$ of $0.01 \mathrm{~N} \mathrm{KMnO}_{4}$
4 $100 \mathrm{~mL}$ of $0.1 \mathrm{~N} \mathrm{KMnO}_{4}$
COMEDK-2011
Chemical Equilibrium

229056 For the reaction $\mathrm{A}+3 \mathrm{~B} \longrightarrow 2 \mathrm{C}+\mathrm{D}$, which one of the following is not correct?

1 Rate of disappearance of $\mathrm{A}=$ Rate of formation of $\mathrm{D}$
2 Rate of formation of $\mathrm{C}=\frac{2}{3} \times$ Rate of disappearance of $\mathrm{B}$
3 Rate of formation of $\mathrm{D}=\frac{1}{3} \times$ Rate of disappearance of $\mathrm{B}$
4 Rate of disappearance of $\mathrm{A}=2 \times$ Rate of formation of $\mathrm{C}$
AP- EAMCET(Medical) -2010
Join With Us for More Updates
Chemical Equilibrium

229049 What is the equilibrium expression for the reaction,

1 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]^5}\)
2 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{5\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]}\)
3 \(\mathrm{K}_{\mathrm{c}}=\left[\mathrm{O}_2\right]^5\)
4 \(\mathrm{K}_{\mathrm{c}}=\frac{1}{\left[\mathrm{O}_2\right]^5}\)
JCECE - 2008
Chemical Equilibrium

229051 Which of the following statements is true when equilibrium is established in the reaction?
$A+B \quad C+D, K_{C}=10$

1 $[\mathrm{C}][\mathrm{D}]=[\mathrm{A}][\mathrm{B}]$
2 $[\mathrm{C}]=[\mathrm{A}]$ and $[\mathrm{B}]=[\mathrm{D}]$
3 $[\mathrm{A}][\mathrm{B}]=0.1[\mathrm{C}][\mathrm{D}]$
4 $[\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=[\mathrm{D}]=10 \mathrm{M}$
AP-EAPCET 24.08.2021 Shift-II
Chemical Equilibrium

229052 For a reaction taking place in three steps, the rate constants are $k_{1}, k_{2}$ and $k_{3}$ and overall rate constant is $k=\frac{k_{1} k_{3}}{k_{2}}$. If the energies of activation $E_{1}, E_{2}$ and $E_{3}$ are 60,30 and $10 \mathrm{~kJ}$ $\mathrm{mol}^{-1}$ respectively, then the overall energy of activation is

1 $30 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $40 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $60 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$
AMU-2014
Chemical Equilibrium

229055 $630 \mathrm{mg}$ of oxalic acid is equivalent to

1 $100 \mathrm{~mL}$ of $0.2 \mathrm{~N} \mathrm{KMnO}_{4}$
2 $100 \mathrm{~mL}$ of $0.05 \mathrm{~N} \mathrm{KMnO}_{4}$
3 $100 \mathrm{~mL}$ of $0.01 \mathrm{~N} \mathrm{KMnO}_{4}$
4 $100 \mathrm{~mL}$ of $0.1 \mathrm{~N} \mathrm{KMnO}_{4}$
COMEDK-2011
Chemical Equilibrium

229056 For the reaction $\mathrm{A}+3 \mathrm{~B} \longrightarrow 2 \mathrm{C}+\mathrm{D}$, which one of the following is not correct?

1 Rate of disappearance of $\mathrm{A}=$ Rate of formation of $\mathrm{D}$
2 Rate of formation of $\mathrm{C}=\frac{2}{3} \times$ Rate of disappearance of $\mathrm{B}$
3 Rate of formation of $\mathrm{D}=\frac{1}{3} \times$ Rate of disappearance of $\mathrm{B}$
4 Rate of disappearance of $\mathrm{A}=2 \times$ Rate of formation of $\mathrm{C}$
AP- EAMCET(Medical) -2010
For More Updates join with Us
Chemical Equilibrium

229049 What is the equilibrium expression for the reaction,

1 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]^5}\)
2 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{5\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]}\)
3 \(\mathrm{K}_{\mathrm{c}}=\left[\mathrm{O}_2\right]^5\)
4 \(\mathrm{K}_{\mathrm{c}}=\frac{1}{\left[\mathrm{O}_2\right]^5}\)
JCECE - 2008
Chemical Equilibrium

229051 Which of the following statements is true when equilibrium is established in the reaction?
$A+B \quad C+D, K_{C}=10$

1 $[\mathrm{C}][\mathrm{D}]=[\mathrm{A}][\mathrm{B}]$
2 $[\mathrm{C}]=[\mathrm{A}]$ and $[\mathrm{B}]=[\mathrm{D}]$
3 $[\mathrm{A}][\mathrm{B}]=0.1[\mathrm{C}][\mathrm{D}]$
4 $[\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=[\mathrm{D}]=10 \mathrm{M}$
AP-EAPCET 24.08.2021 Shift-II
Chemical Equilibrium

229052 For a reaction taking place in three steps, the rate constants are $k_{1}, k_{2}$ and $k_{3}$ and overall rate constant is $k=\frac{k_{1} k_{3}}{k_{2}}$. If the energies of activation $E_{1}, E_{2}$ and $E_{3}$ are 60,30 and $10 \mathrm{~kJ}$ $\mathrm{mol}^{-1}$ respectively, then the overall energy of activation is

1 $30 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $40 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $60 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$
AMU-2014
Chemical Equilibrium

229055 $630 \mathrm{mg}$ of oxalic acid is equivalent to

1 $100 \mathrm{~mL}$ of $0.2 \mathrm{~N} \mathrm{KMnO}_{4}$
2 $100 \mathrm{~mL}$ of $0.05 \mathrm{~N} \mathrm{KMnO}_{4}$
3 $100 \mathrm{~mL}$ of $0.01 \mathrm{~N} \mathrm{KMnO}_{4}$
4 $100 \mathrm{~mL}$ of $0.1 \mathrm{~N} \mathrm{KMnO}_{4}$
COMEDK-2011
Chemical Equilibrium

229056 For the reaction $\mathrm{A}+3 \mathrm{~B} \longrightarrow 2 \mathrm{C}+\mathrm{D}$, which one of the following is not correct?

1 Rate of disappearance of $\mathrm{A}=$ Rate of formation of $\mathrm{D}$
2 Rate of formation of $\mathrm{C}=\frac{2}{3} \times$ Rate of disappearance of $\mathrm{B}$
3 Rate of formation of $\mathrm{D}=\frac{1}{3} \times$ Rate of disappearance of $\mathrm{B}$
4 Rate of disappearance of $\mathrm{A}=2 \times$ Rate of formation of $\mathrm{C}$
AP- EAMCET(Medical) -2010
NEET DIGITAL LIBRARY
Chemical Equilibrium

229049 What is the equilibrium expression for the reaction,

1 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]^5}\)
2 \(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{P}_4 \mathrm{O}_{10}\right]}{5\left[\mathrm{P}_4\right]\left[\mathrm{O}_2\right]}\)
3 \(\mathrm{K}_{\mathrm{c}}=\left[\mathrm{O}_2\right]^5\)
4 \(\mathrm{K}_{\mathrm{c}}=\frac{1}{\left[\mathrm{O}_2\right]^5}\)
JCECE - 2008
Chemical Equilibrium

229051 Which of the following statements is true when equilibrium is established in the reaction?
$A+B \quad C+D, K_{C}=10$

1 $[\mathrm{C}][\mathrm{D}]=[\mathrm{A}][\mathrm{B}]$
2 $[\mathrm{C}]=[\mathrm{A}]$ and $[\mathrm{B}]=[\mathrm{D}]$
3 $[\mathrm{A}][\mathrm{B}]=0.1[\mathrm{C}][\mathrm{D}]$
4 $[\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=[\mathrm{D}]=10 \mathrm{M}$
AP-EAPCET 24.08.2021 Shift-II
Chemical Equilibrium

229052 For a reaction taking place in three steps, the rate constants are $k_{1}, k_{2}$ and $k_{3}$ and overall rate constant is $k=\frac{k_{1} k_{3}}{k_{2}}$. If the energies of activation $E_{1}, E_{2}$ and $E_{3}$ are 60,30 and $10 \mathrm{~kJ}$ $\mathrm{mol}^{-1}$ respectively, then the overall energy of activation is

1 $30 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $40 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $60 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$
AMU-2014
Chemical Equilibrium

229055 $630 \mathrm{mg}$ of oxalic acid is equivalent to

1 $100 \mathrm{~mL}$ of $0.2 \mathrm{~N} \mathrm{KMnO}_{4}$
2 $100 \mathrm{~mL}$ of $0.05 \mathrm{~N} \mathrm{KMnO}_{4}$
3 $100 \mathrm{~mL}$ of $0.01 \mathrm{~N} \mathrm{KMnO}_{4}$
4 $100 \mathrm{~mL}$ of $0.1 \mathrm{~N} \mathrm{KMnO}_{4}$
COMEDK-2011
Chemical Equilibrium

229056 For the reaction $\mathrm{A}+3 \mathrm{~B} \longrightarrow 2 \mathrm{C}+\mathrm{D}$, which one of the following is not correct?

1 Rate of disappearance of $\mathrm{A}=$ Rate of formation of $\mathrm{D}$
2 Rate of formation of $\mathrm{C}=\frac{2}{3} \times$ Rate of disappearance of $\mathrm{B}$
3 Rate of formation of $\mathrm{D}=\frac{1}{3} \times$ Rate of disappearance of $\mathrm{B}$
4 Rate of disappearance of $\mathrm{A}=2 \times$ Rate of formation of $\mathrm{C}$
AP- EAMCET(Medical) -2010