Practice ProblemATTEMPT
For each change indicated, determine whether the equilibrium:
will shift to the right, shift to the left, or neither: (a) addition of
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Chemistry
- Please see attached image for Chemistry problem question Thank youarrow_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_forwardPractice chemistry questionarrow_forward
- answer should be all valid numeric valuearrow_forwardQuestion 21 Hydrogen iodide can be produced by the reversible reaction of hydrogen gas and iodine gas according to: H2(g) + I2(g) = 2HI(g) Keg for this reaction is 2.25 × 10³ at a temperature of 753°C. Calculate the concentration of HI in an equilibrium mixture if the concentration of H2 is 0.15 M and the concentration of I2 is 0.25 M. (a) 2.4 moles of H2(g) and 1.5 moles of I2(g) were placed in a sealed 2.0 L vessel maintained at a temperature of 753°C. After 2 hours, the number of moles of each gas present were as follows. (b) Moles of H2(g) Moles of I2(g) Moles of HI(g) 1.7 0.8 1.4 Show by calculation whether the forward or reverse reaction must increase for the system to come to a state of dynamic equilibrium.arrow_forwardConsider 4 NH3(g)+ 5 O2(g)⇋4 NO(g)+ 6 H2O(g)(ΔH = -904.4 kJ). How does each of the following changes affect the yield of NO at equilibrium? Answer increase, decrease, or no change. (a)Increase [H2O] (b)Decrease [O2] (c)Decrease the volume of the container in which the reaction occurs .(d)Add a catalyst. (e)Increase temperaturearrow_forward
- Select all that apply. For the following equilibrium system, which of the following changes will form more CaCO3? CO2(g) + Ca(OH)2(s) = CaCO3(s) + H2O(l) 0 ΔΗ =-113 kJ rxn Decrease temperature at constant pressure (no phase change). Increase volume at constant temperature. Increase partial pressure of CO2. Remove one-half of the initial CaCO3.arrow_forwardPlease correct answer and don't use hand raitingarrow_forwardQuestion 2 Consider the following reactions, with equilibrium contants as shown: (1) C(s) + 0,(g) co,(g), K, (2) 2Ca(s) + O,(g)=2CaO(s). K, (3) 2Ca(s) + 2C(s) + 30,(g) =2CaCO,(s), K, In terms of K1, K2 and K3 , the equilibrium constant for the reaction CaO (s) +CO,(g) CACO,(s) can be expressed as: O a. O b. (K,) 2 + (K, + (K c. Od. O e. ) ( f. + (K None of the above.arrow_forward
- e) 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_forwardQuestion attachedarrow_forwardK=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_forward
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