NEET Questions - Chemistry

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Three gaseous equilibria have values of equilibrium constants as $k_1 , k_2, k_3 $ . resp. (i) $ A +B \rightleftharpoons C $ (ii) $ B+C \rightleftharpoons P+Q $ (iii) $ A+2B \rightleftharpoons P+Q $. What is the relation between $k_1 ,k_2, k_3$ . (?)

K_3 = K_1 / K_2
$ K_3 = { K_1 \times K_2 } $
$ K_1 = K_2 \times K_3 $
$ K_1 \times K_2 \times K_3 = 1 $

Three gaseous equilibria have value of equilibrium constants as $K_1, K_2 , K_3$ respectively. (i)$ N_2 + O_2 \rightleftharpoons 2 NO (K_1) $ (ii) $ N_2 + 2O_2 \rightleftharpoons 2 NO_2 (K_2 ) $ (iii) $ 2NO +2 O_2 \rightleftharpoons 2 NO_2 (K_3 ) $ What is the relation between $ K_1, K_2 and K_3 (?) $

$ K_3 = K_1 \times K_2 $
$ K_1 = K_2 \times K_3 $
$ K_2 = K_1 \times K_3 $
$ K = K_1 \times K_2 \times K_3 $

The equilibrium constant for the reaction, $ N_{2(g)} + O_{2(g) } \rightleftharpoons 2 NO_{(g)} is 4.4 \times 10 ^ {-4 } $ at 2000k temp In presence ofa catalyst, equilibrium is attained ten times faster. Therefore the equilibrium constant, in presence of catalyst at 2000K is........

$ 4.4 \times 10 ^ {-4} $
$ 4.4 \times 10 ^ {-5} $
$ 4.4 \times 10 ^ {-3} $
difficult to compute

For the following reaction in gaseous phase $ CO + 1/2 O_2 \rightleftharpoons CO_2 $ $ KC/ KP $ is

$ ( RT) ^ {1/2} $
$ ( RT) ^ { -1/2} $
RT
$ ( RT)^{-1} $

For the reaction equilibrium, $ N_2O_{4(g )} \rightleftharpoons 2NO_{( g)} the concentration of N_2O_4 and NO_2 at equilibrium are 4.8 \times 10 ^ {-2} and 1.2 \times 10 ^ {-2} molL^{-1} respectively. The value of K_C $ for the reaction is :

$ 3.3\times 10^2 mol L ^{-1} $
$ 3\times 10^1 mol L ^{-1} $
$ 3 \times 10^{-3 }mol L ^{-1}$
$ 3\times 10^3 mol L ^{-1} $

Which one of the following statements is not true ?

The conjugate base of $ H_2 PO_4 ^ - is HPO_4 ^ {2-} $
$ P ^ H + P ^ {OH} = 14 for all aqueous solutions at 298 K $
$ P ^ H of 1 \times 10 ^ {-8} M HCl is 8 $
$ NH_3 $ is a lewis base

What is the equilibrium expression for the reaction. $ P_{4(s)} + 5O_{2(g)} \rightleftharpoons P_4O_{10(s)} $

$ Kc = {{ [ P_4 O_{10}] }\over [ P_4] [ O_2] ^ 5 }$
$ Kc = {1 \over [ O_2] ^ 5 }$
$ Kc = {{ [ P_4 O_{10}] }\over 5[ P_4] [ O_2] }$
$ Kc = { [ O_2] ^ 5 }$

For the reaction CO(g) + Cl2(g) ----> COCl2(g) then Kp/ Kc is equal to

$ { 1 \over RT} $
RT
$ \sqrt { RT} $
1

The equilibrium constant for the reaction $ N_{2(g)} + O_{2(g)} \rightleftharpoons 2 NO_{(g)} at temperature. 300 k is 4 \times 10^{-4 } $.The value of Kc for the reaction $ NO_{(g)} \rightleftharpoons {1 /2 } N_{2(g) } + { 1/2} O_{2(g) } $ at the same temperature is

$ 2.5 \times 10 ^ 2 $
$ 4 \times 10 ^ {-4} $
0.02
50

Hydrogen ion concentration in mol/ L in a solution of $ P^H = 5.4 $ will be,

$ 3.98 \times 10 ^ {-6} $
$ 3.68 \times 10 ^ {-6} $
$ 3.88 \times 10 ^ 6 $
$ 3.98 \times 10 ^ 8 $

$ In a reaction, CO_{(g)} + 2H_{2(g)} \rightleftharpoons CH_{(g)} OH \triangle H^ \circ = -92 KJ mol ^ {-1 } $ concentration of hydrogen,carbon monoxide and methanol become constant at equilibrium. what willhappen if an inert gas is added to the system.?

reaction becomes fast
reaction becomes slow
equilibrium state disturbs
equilibrium state remains undisturbed

At 473 k, equilibrium constant $ K_C for the reaction PCl_{5(s)} \rightleftharpoons PCl_{3(g)}+ P Cl_{2(g)} is 8.3 \times 10 ^ {-3} what is the value of K_C $ for the reverse reaction at the same temperature ?

$ 8.3\times 10 ^ {-3} $
120.48
$ 16.6 \times 10 ^ {-3} $
$ 4.15 \times 10 ^ {-3} $

At 473 k, equilibrium constant KC for a reaction, $ PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)} is 8.3 \times 10 ^ {-3 } ( \triangle H = 124 Kjmol ^{-1 }) $ What would be the effect on $ K_C $ if (i) more PCls is added (ii) the pressure is increased (iii) the temp is increased

$ K_c $ remains unchanged, unchanged, increase.
$ K_c $ increases, increases, decreases.
$ K_c $ remains unchanged, increase, unchanged.
$ K_c $ decreases, increases, unchanged.

The equilibrium constant for the reaction $ N_{2(g)} + O_{2(g)} \rightleftharpoons 2 NO_{(g)} is 4 \times 10 ^ {-4} at 2000K temperature. what is the value of kc for the reaction 3/2 N_{2(g)} + 3/2 O_{2 (g)} \rightleftharpoons 3 NO_{(g)} $

$ 4 \times 10 ^ {-4} $
$ 8 \times 10 ^ {-6} $
$ 8 \times 10 ^ {-4} $
$ 16 \times 10 ^ {-4} $

For the reversible reaction $ N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} at 500 \circ c the value of K_P is 1.44 \times 10 ^{-5} $ . what would be the value of KC for the same reaction

$ 1.44 \times 10 ^ 5 / (0.082 \times 500)^{-2} $
$ 1.44 \times 10 ^{- 5} / (8.314 \times 773)^{-2} $
$ 1.44 \times 10 ^{- 5} / (0.082 \times 773)^{2} $
$ 1.44 \times 10 ^ {-5 } / (0.082 \times 773)^{-2} $

NEET Chemistry Questions: Equilibrium