Oxidation state of nitrogen is correctly given for :

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For the reaction $A(g)+B(g) \rightleftharpoons C(g)$ at equilibrium, the partial pressure of the species are $P_{A}=0.15$ atm, $P_{C}=P_{B}=0.30$ atm.

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The graph which will be representing all the equilibrium concentrations for the reaction —

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For the reaction: H2(g)+ I2(g) $\rightleftharpoons$ 2HI (g), the equilibrium constant $K _{ p }$ changes with :

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The equilibrium constant for the reaction —

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Two elements X (at. mass =16) and Y (at. mass =14) combine to form compounds A, B and C. The ratio of different masses of Y which combines with a fixed mass of X in A, B and C is 1: 3: 5.

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	Compound	Oxidation State
(D)	H₂N₂O₂	+1

Oxidation state of nitrogen is correctly given for :

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