Calculate the value of the equilibrium constant, K., for the reaction Q(g)+X(g) 2 M(g)+N(g) given that M(g) Z(g) 6 R(g) 2 N(g) + 4Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kel = 3.12 K2 = 0.412 Ke3 Kc3 = 14.2
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- A reaction mixture that consisted of 0.20 mol N2(g) and 0.20 mol H2(g) was introduced into a reactor of volume 25.0 L and heated. At equilibrium, 5.0% of the nitrogen gas had reacted. What is the value of the equilibrium constant KC for the reaction N2(g) + 3H2(g) ⇋ 2 NH3(g) at this temperature?Calcium hydroxide is a base that does not dissolve very well in water. When saturated, a calcium hydroxide solution at 25°C contains 1,3 gram Ca(OH)2 per dm3 solution. The molar mass of Ca(OH)2 is 74,1 g×mol–1. When the Ca(OH)2 dissolves, the following reaction represents the solubility equilibrium: Ca(OH)2 (s) D Ca2+ (aq) + 2 OH– (aq) Use this information above to find the value of Ksp for Ca(OH)2 at 25°C.Calcium hydroxide is a base that does not dissolve very well in water. When saturated, a calcium hydroxide solution at 25°C contains 1,3 gram Ca(OH)2 per dm3 solution. The molar mass of Ca(OH)2 is 74,1 g×mol–1. When the Ca(OH)2 dissolves, the following reaction represents the solubility equilibrium: Ca(OH)2 (s) D Ca2+ (aq) + 2 OH– (aq) Use this information above to find the value of Ksp for Ca(OH)2 at 25°C. What is the pH of this saturated Ca(OH)2 solution?
- The following synthesis reaction was conducted at 325K: A2(g) + 3B2(g) ⇌ 2AB3(g). At this temperature, KP = 5.49 x 10-6. In a 3.00L flask, 0.175atm of A2(g) and 0.410atm of B2(g) are added and allowed to reach equilibrium. Calculate the pressure of AB3(g) in the system (in atm).Write the expression for Keq for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. H2(g) + I2(g) 2 HI(g) Keq = 2 PHI / (PH2 PI2) Keq = PH2 PI2 / 2 PHI Keq = PH2 PI2 / PHI2 Keq = PHI2 / (PH2 PI2)Consider a body of water in equilibrium with solid calcium sulfate, CaSo4, for which Ksp= 3.0 x 10^-5 at 25 degrees C. Calculate the solubility, in g/L, of calcium sulfate in water assuming that other reactions are negligible. *
- Estimate the temperature at which the equilibrium constant for CuSO4 ⋅ 5 H2O(s) → CuSO4(s) + 5 H2O(g) becomes 1; assume pH2O = 1 bar.A student determines the molar mass of acetone by the method used in this experiment. She found that the equilibrium temperature of a mixture of ice and water was 0.5 C on her thermometer. When she added 10.5 g of her sample to the mixture, the temperature fell to -3.7 C. She then poured off the solution through a screen into a beaker. The mass of the solution was 86.4 g. How much acetone was in the decanted solution?Calculate the equilibrium constant at 37°C for the reaction Glucose +6O2 + 36ADP + 36Phosphate -> 6CO2 + 42H2O + 36ATP Change in G°= -423kcal/mole of Glucose
- Consider a body of water in equilibrium with solid calcium sulfate, CaSO4, for which Ksp = 3.0 * 10^-5 at 35 degrees C. Calculate the solubility, in g/L of calcium sulfate in water assuming that other reactions are negligible.In the Harber process for ammonia synthesis, K= 0.036 for N2(g) + 3H2(g) ⇋ 2 NH3(g) at 500. K. If the reactor of vlume 2.0 L charged with 1.42 bar N2 and 2.87 bar H2, what will the equilibrium partial pressures in the mixture?It was determined by spectrophotometry that the moles of FeSCN2+ present at equilibrium was 2.00 x 10-4 moles (2.00 times 10 to the minus 4th power moles). If the sample was prepared using 4.00 x 10-3 moles (4.00 times 10 to the minus 3rd power moles) of Fe3+, how many moles of Fe3+ were present at equilibrium?