Ans.
Reaction :
2HBr(g) + 72.7 KJ <----> H2(g) + Br2(g)
As heat is added in the reaction , so , this reaction is endothermic reaction
According to Le Chatelier's principle , in an endothermic reaction , when temperature is increased , the equilibrium will shift to the right side
Therefore , answer is (B) , right , and the concentration of HBr(g) will decrease
35) Given the equilibrium reaction at constant pressure: 2HBr(g) + 72.7 kJ = H2(g) + Br2(g)...
The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.20 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 9.20 atm of HBr is introduced into a sealed container at this temperature.
The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.35 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 5.70 atm of HBr is introduced into a sealed container at this temperature.
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The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 1.20 moles of HBr in a 21.3−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium.
M. Given the system at euo N04g)+58.1 kJ+2 NOg) 14. Given the reaction at equilibrium: what will be the result ofan increase in temperature | at constant pressure? |NaCo) + hola) +21.6 kcal ++ NO(g) A) The equilibrium wil shift to the left, and the The equilibrium will shift to the right if the A) temperature increases B) temperature decreases C) pressure increases D) pressure decreases concentration of NO2(g) will decrease. B) The equilibrium will shift to the left, and...
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The value of the equilibrium constant for the reaction 2HBr(g)<....>H2(g)+Br2(g) is Kc=1.26*10^-12 at 500k. A. what would be the value of the equilibrium constant K'c for the related reaction written in the following fashion? 1/2 H2(g)+1/2 Br2(g)<....>HBr(g). B. what will be the corresponding value for Kp, the pressure form of the equilibrium constant? (R=0.08206)
please show work for these problems, correct answers are circled 26. Consider the reaction: 2HBr(g) = H2(g) + Br2(g) Keq = 49.0 If 1.20 M H2, 1.20 M Br2 and 1.00 M HBr are placed into a container at 44° C, which of the following is true as equilibrium is approached? A. [Br2] decreases significantly. B. [HBr] decreases significantly. C. [H2] decreases significantly. D. [H2) remains the same. 27. Which Keq is most likely to favour the formation of reactants?...
The molar equilibrium constant, Kc, is 7.7x10-11at 25oC for the reaction: 2HBr(g) <--> H2(g)+ Br2(g) What is the gas-phase equilibrium constant, Kp, for the reaction: Br2(g)+ H2(g) <--> 2HBr(g) a. 1.8x10-9 b. 7.7x10-11 c. 0.0 d. 1.3x1010 e. 3.8x1011