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Sahay Sir > Question Answers > NCERT Exemplar Class 11 > Chemistry > Chapter 7 - Equilibrium > The equilibrium constant for the following reaction is 1.6×10^5 at 1024K H2(g)+Br2(g)⇔2HBr(g) find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024K.

The equilibrium constant for the following reaction is 1.6×10^5 at 1024K H2(g)+Br2(g)⇔2HBr(g) find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024K.

2.0 mol litre^−1 H2 ​ and 0.5 mol litre^−1 NH3. Is the reaction at equilibrium? If not Equilibrium constant in which direction does the reaction tend to proceed to reach equilibrium? Kc for the reaction n2 N2(g)+3H2(g) ⇌ 2NH3(g) ; at 500 K is 0.061 litre 2 mole^−2. At a particular time the analysis shows that composition of the reaction mixture is 3.00 mol litre^−1