Consider the following reaction: 2H2S(g)+SO2(g)⇌3S(s)+2H2O(g) A reaction mixture initially containing 0.480 M H2S and 0.480 M SO2 was found to contain 1.3×10−3 M H2O at a certain temperature. A second reaction mixture at the same temperature initially contains [H2S]= 0.255 M and [SO2]= 0.325 M . Part A Calculate the equilibrium concentration of  H2O  in the second mixture at this temperature

53. For the reaction, Kc=0.513Kc=0.513 at 500 K. N2O4(g)⇌2 NO2(g)N2O4(g)⇌2 NO2(g) If a reaction vessel initially contains an N2O4N2O4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations of N2O4N2O4 and NO2NO2 at 500 K?

The following reaction was initiated with NOCl(g), with a partial pressure of NOCl(g) = 0.66 atm. The reaction achieved equilibrium at 25⁰C where equilibrium partial pressure for NOCl(g) : (?????(?) ) = 0.33 atm. Calculate the KC value for this reaction. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) A) 3.3 × 10-4 B) 0.165 C) 3.3 D) 6.74 × 10-3 E) 0.0042 atm

The value of K, for the reaction 2 NO, (g) N204 (g) is 1.52 at 319 K. What is the value of the Kp of the reaction NO2 (g) 1/2 N204 (g) at this temperature: 0.761 O2.31 1.23 1.52 0.811 A Moving to another question will save this response. Esc AI C 中 F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 23 %24

In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC.  In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first.  This mixture is also heated to 350 oC.  After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?

Consider the following reaction: 2 SO2(g) + O2(g) ⇋ 2 SO3(g); Keq = 4.34 at 600°C An equilibrium mixture of this reaction contains [O2] = 0.125 M and [SO3] = 0.391 M at 600°C. What is [SO2]?

As shown in Table 15.2 in the textbook, KpKp for the equilibriumN2(g)+3H2(g)⇌2NH3(g)N2(g)+3H2(g)⇌2NH3(g)is 4.51×10−54.51×10−5 at 450 ∘C∘C. For each of the mixtures listed here, indicate whether the mixture is at equilibrium at 450 ∘C∘C. If it is not at equilibrium, indicate the direction (toward product or toward reactants) in which the mixture must shift to achieve equilibrium. A. 98 atmatm NH3NH3, 45 atmatm N2N2, 55 atmatm H2H2 98  , 45  , 55   a. yes, mixture is at equilibrium b. no, mixture must shift toward products to achieve equilibrium c. no, mixture must shift toward reactants to achieve equilibrium B.57 atmatm NH3NH3, 143 atmatm N2N2, no H2H2 57  , 143  , no  a.yes, mixture is at equilibrium b.no, mixture must shift toward products to achieve equilibrium c.no, mixture must shift toward reactants to achieve equilibrium

3. Consider the reaction Br2 (g) + Cl2 (g) 2 BrCl (g) Kp = 1.11 x 104 at 150 K. A reaction mixture initially contains a Br2 partial pressure of 0.993 atm and a Cl2 partial pressure of 0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product. 4. Consider the reaction CO₂ (g) + H2 (g) A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product. CO (g) + H₂O (g) Kp = 0.0611 at 2000K.

For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) Kp = 1.40×10−3 at a certain temperature. A flask is charged with 50.7 kPa PCl3 What are the equilibrium partial pressures of PCl3 , Cl2 , and PCl5 , respectively? , 50.7 kPa Cl2 , and 30.4 kPa PCl5 at this temperature.