Equilibrium practice · Medium

In a lime kiln, to get higher yield of $\mathrm{C}{\mathrm{O}_2}$, the measure that can be taken is

A white salt is readily soluble in water and gives a colourless solution with a pH of about 9. The salt would be:

In a reaction $PC{l_5}PC{l_3} + C{l_2}$, degree of dissociation is 30%, If initial moles of $PC{l_5}$ is one then total moles at equilibrium is

0.1 mole of ${\mathrm{N}_2}{\mathrm{O}_4}\left( \mathrm{g} \right)$ was sealed in a tube under one atmospheric conditions at $25^\circ C$. Calculate the number of moles of $\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)$ present, if the equilibrium ${\mathrm{N}_2}{\mathrm{O}_4}\left( \mathrm{g} \right)\;\leftrightharpoons\;2\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)\left( {{K_p} = 0.14} \right)$ is reached after some times

Which is decreasing order of strength of bases?
$\mathop \mathrm{O}\limits^\_ \mathrm{H},\mathop \mathrm{N}\limits^\_ {\mathrm{H}_2},\mathrm{HC} \equiv {\mathrm{C}^ - }\mathrm{and C}{\mathrm{H}_3}\mathrm{CH}_2^ -$

For the reaction
$2S{O_2}(g) + {O_2}(g) \to 2S{O_3}(g),\Delta H = - 57.2\mathrm{kJ}\,\mathrm{mo}{\mathrm{l}^{ - 1}}\mathrm{ and }{K_c} = 1.7 \times {10^{16}}$
Which of the following statement is incorrect?

The equilibrium which remains unaffected by change in pressure of the reactants is

When ${10^{ - 8}}$ mole of $\mathrm{HCl}$ is dissolved in one litre of water, the $\mathrm{pH}$ of the solution will be:

A physician wishes to prepare a buffer solution at $\mathrm{pH} = 3.58$ that efficiently resists a change in $\mathrm{pH}$ yet contains only small conc. of the buffering agents. Which one of the following weak acid together with its sodium salt would be best to use?

In which of the following cases, does not reaction go farthest to completion?

When $20\;g$ of $\mathrm{CaC}{\mathrm{O}_3}$ were put into $10\;\mathrm{ }litre$ flask and heated to $800^\circ C$, $35\%$ of $\mathrm{CaC}{\mathrm{O}_3}$ remained unreacted at equilibrium. ${K_p}$ for decomposition of $\mathrm{CaC}{\mathrm{O}_3}$ is :

For the gaseous phase reaction, $2NO\leftrightharpoons{N_2} + \mathrm{ }{O_2}$, $\Delta {H^ \circ } = \mathrm{ } - \mathrm{ }43.5\mathrm{ }\;k\;cal\mathrm{ }\;mo{l^{ - 1}},$  which statement is correct for, ${N_2}\left( g \right)\mathrm{ } + \mathrm{ }{O_2}\left( g \right)\mathrm{ }\leftrightharpoons\mathrm{ }2NO\left( g \right)?$

For the following Assertion and Reason the correct option is
Assertion: The pH of water increases with increase in temperature.
Reason: The dissociation of water into ${H^ + }$ and $O{H^ - }$ is an exothermic reaction.

The following reactions are known to occur in the body,

$\mathrm{C}{\mathrm{O}_2} + {\mathrm{H}_2}\mathrm{O}\leftrightharpoons{\mathrm{H}_2}\mathrm{C}{\mathrm{O}_3}\leftrightharpoons{\mathrm{H}^ + } + \mathrm{HCO}_3^ -$

If $\mathrm{C}{\mathrm{O}_2}$ escapes from the system, then:

pH of 0.2 M aqueous solution of sodium benzoate will be ($P{K_a}$ of benzoic acid = 4.2)

The concentration of $\mathrm{C}{\mathrm{O}_2}$ be in equilibrium with $2.5 \times {10^{ - 2}}\;\mathrm{mol}\;\mathrm{ litr}{\mathrm{e}^{ - 1}}\;\mathrm{of }\;\mathrm{CO}\;\mathrm{at}\,\,100^\circ C$ for the reaction : $\mathrm{FeO}\left( s \right)\; + \,\,\mathrm{CO}\left( \mathrm{g} \right)\;\,\leftrightharpoons\;\mathrm{Fe}\left( s \right) + \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right);\;{K_c} = 5.0$

STATEMENT I : pH value of acidic buffer solution change, k if bufler solution is diluted upto very larger extent.

STATEMENT II : $\left[H^{+}\right]$ decrease due to change in concentration as well as $\alpha$ and decrease in concentration is more as compare to increase in $\alpha$.

$100\;\mathrm{ }mL\;\mathrm{ }of\;\mathrm{ }0.01\mathrm{ }M$ solution of $\mathrm{NaOH}$ is diluted to $1\;\mathrm{d}{\mathrm{m}^3}$. What is the pH of the diluted solution?

The decreasing order of strength of the bases,

$\mathrm{O}{\mathrm{H}^ - },\mathrm{NH}_2^ - ,\mathrm{H}-\mathrm{C} \equiv {\mathrm{C}^ - }\;and\;\mathrm{C}{\mathrm{H}_3}-\mathrm{CH}_2^ - ,\;is$

The internal and external indicator among the following respectively are:

Arrange $\mathrm{NH}_4^ + ,{\mathrm{H}_2}\mathrm{O},{\mathrm{H}_3}{\mathrm{O}^ + },\mathrm{HF }\;\mathrm{and}\;\mathrm{ O}{\mathrm{H}^ - }$ in increasing order of acidic nature

4 moles of A is mixed with 4 moles of B, at equilibrium for the reaction $A + BC + D$, 2 moles of C and D is formed. The equilibrium constant for the reaction will be

In a reaction at equilibrium $'X'$ mole of the reactant $A$ decompose to give $1\;mole$ each of $C\;and\;D$ . If the fraction of $A$ decomposed at equilibrium is independent of initial concentration of $A$, then the value of $'X'$ is :

Which of the following has ${P^H}$ is equal to near about one

What is equilibrium expression for the reaction, ${P_4}(s) + 5{O_2}(g)\leftrightharpoons{P_4}{O_{10}}(s)\,\,?$

For the system; $3A + 2B\leftrightharpoons\;C$,the expression for equilibrium constant is

A cylinder fitted with a movable piston contains liquid water in equilibrium with water vapour at 250C. Which operation result in a decrease in the equilibrium vapour pressure?

The equilibrium constant for the reaction between $C{H_4}\left( g \right)$ and ${H_2}S\left( g \right)$ to form $C{S_2}\left( g \right)$ and ${H_2}\left( g \right)$ , at 1173 K is 3.6. For the following composition of the reaction mixture, $\left[ {C{H_4}} \right] = 1.0\,M,\,\left[ {{H_2}S} \right] = 1.20M\,\,\,\left[ {C{S_2}} \right] = 2.0M,\,\,\left[ {{H_2}} \right] = 1.8M$ decide which of the following option is correct? $\left[ {C{H_4}\left( g \right) + 2{H_2}S\left( g \right)C{S_2}\left( g \right) + 4{H_2}\left( g \right)} \right]$

The buffering action of an acidic buffer is maximum when its $pH$ is equal to

For which of the following reactions,${K_p} = {K_c}$ ?