1

JEE Main 2021 (Online) 27th August Evening Shift

Numerical

+4

-1

When 5.1 g of solid NH

_{4}HS is introduced into a two litre evacuated flask at 27$$^\circ$$C, 20% of the solid decomposes into gaseous ammonia and hydrogen sulphide. The K_{p}for the reaction at 27$$^\circ$$C is x $$\times$$ 10^{$$-$$2}. The value of x is _____________. (Integer answer) [Given R = 0.082 L atm K^{$$-$$1}mol^{$$-$$}]Your input ____

2

JEE Main 2021 (Online) 27th August Morning Shift

Numerical

+4

-1

The number of moles of NH

[Assume no volume change on adding NH

_{3}, that must be added to 2L of 0.80 M AgNO_{3}in order to reduce the concentration of Ag^{+}ions to 5.0 $$\times$$ 10^{$$-$$8}M (K_{formation}for [Ag(NH_{3})_{2}]^{+}= 1.0 $$\times$$ 10^{8}) is ____________. (Nearest integer)[Assume no volume change on adding NH

_{3}]Your input ____

3

JEE Main 2021 (Online) 26th August Evening Shift

Numerical

+4

-1

The equilibrium constant K

_{c}at 298 K for the reaction A + B $$\rightleftharpoons$$ C + D is 100. Starting with an equimolar solution with concentrations of A, B, C and D all equal to 1M, the equilibrium concentration of D is ___________ $$\times$$ 10^{$$-$$2}M. (Nearest integer)Your input ____

4

JEE Main 2021 (Online) 26th August Evening Shift

Numerical

+4

-1

The reaction rate for the reaction

[PtCl

was measured as a function of concentrations of different species. It was observed that $${{ - d\left[ {{{\left[ {PtC{l_4}} \right]}^{2 - }}} \right]} \over {dt}} = 4.8 \times {10^{ - 5}}\left[ {{{\left[ {PtC{l_4}} \right]}^{2 - }}} \right] - 2.4 \times {10^{ - 3}}\left[ {{{\left[ {Pt({H_2}O)C{l_3}} \right]}^ - }} \right]\left[ {C{l^ - }} \right]$$.

where square brackets are used to denote molar concentrations. The equilibrium constant K

[PtCl

_{4}]^{2$$-$$}+ H_{2}O $$\rightleftharpoons$$ [Pt(H_{2}O)Cl_{3}]^{$$-$$}+ Cl^{$$-$$}was measured as a function of concentrations of different species. It was observed that $${{ - d\left[ {{{\left[ {PtC{l_4}} \right]}^{2 - }}} \right]} \over {dt}} = 4.8 \times {10^{ - 5}}\left[ {{{\left[ {PtC{l_4}} \right]}^{2 - }}} \right] - 2.4 \times {10^{ - 3}}\left[ {{{\left[ {Pt({H_2}O)C{l_3}} \right]}^ - }} \right]\left[ {C{l^ - }} \right]$$.

where square brackets are used to denote molar concentrations. The equilibrium constant K

_{c}= ____________ . (Nearest integer)Your input ____

Questions Asked from Chemical Equilibrium (Numerical)

Number in Brackets after Paper Indicates No. of Questions

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