Practice Problem BUILD
Consider a weak acid, HA, that ionizes according to the equation:
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Chemistry
- K=4.9x10-3 for the reaction CO2(g)+H2(g)⇄ CO(g)+H2O(g). If [CO2]=0.00025 M, [H2]=0.0010 M, & [CO]=0.000015 M, what is the concentration at equilibrium of H2O? Answer 8.2x10-5M I got 1.84x10^-14? Can someone explain this to me please.arrow_forward9. The equilibrium constant for the reaction 2 BrCl (g) → Br2 (g) + Cl2 (g) at 25°C is Keq = 0.0172. What is the equilibrium constant for the reaction Br2 (g) + Cl2 (g) →2 BrCl (g)? (а) -0.0172 (b) 0.131 (c) 7.62 (d) 58.1 (e) none of thesearrow_forwarde) none of the above 25. If K = 0.124 for A2 + 2B = 2AB, what is the value of K, for the reaction 4AB 2A2 + 4B? a) 0.124 b) 0.248 c) 65.0 d) – 0.124 e) 4.03 f) none of the abovearrow_forward
- (Incorrect) For the reaction 2A(g) + B(s) C() + 2D(g) at 700 °C, Kc = 0.00577. Calculate the number of moles of D present at equilibrium if a mixture of 6.03 moles of C and 6.03 moles of D is heated to 700 °C in a 7.61-L container. 0.0074 mol (Your answer) 0.430 mol (Correct answer) 5.60 mol 0.056 molarrow_forwardThe equilibrium constant for the equilibrium, 3A+ 2B ↔ 2D + E, is 4.22 x 10-3 . What is the equilibrium constant for the equilibrium: D + (1/2)E ↔ (3/2)A + B? (a)237 (b)2.11×10-3 (c)15.4 (d)-2.11×10-3arrow_forwardTUTOR Calculate K from Equilibrium Concentrations Some SO, is placed in a sealed flask and heated to 1350 K. When equilibrium is reached, the flask is found to contain SO3 (6.00×10 M), SO, (3.47x102 M), and O2 (1.59×10-² M). What is the value of the equilibrium constant for this reaction at 1350 K? 2S03(g) 2SO2(g) + O2(g) K=arrow_forward
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