In which of the following reactions will Kc = Kp? 4 NH_3 (g) + 3 O_2...
For the following equilibrium: N_2(g) + H_2(g) rightarrow NH_3(g) delta H= -386 kJ/mole Predict the direction the equilibrium will shift if: N_2 is added? H_2 is removed? NH_3 is added? NH_3 is removed? the volume of the container is decreased? the pressure is increased by adding Argon gas? the reaction is cooled? equal number of moles of H_2 and NH_3 are added? a catalyst is added The equilibrium constant for the following reaction is 5.0 at 400 degree C. CO_(g)...
At a certain temperature, the following reactions have the equilibrium constants shown. S(s) + O_2(g) rightwardsharpoonoverleftwardsharpoon SO_2(g) K_c = 10^2S(s) + 3O_2(g) rightwardsharpoonoverleftwardsharpoon 2SO_2(g) k_ = 9.8 times 10^Calculate the equilibrium constant, K_c. for the following reaction at that temperature. 2SO_2(g) + O_2(g) rightarrow 2SO_3(g)
14. In which of the following reactions will Kc = Ko? ooo 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(g) 2 SO3(g) + 2 NO(g) = 2 SO2(g) + 2 NO2(g) 4 N2(g) + 2 O2(g) = 4 N2O(g) 6 SO2(g) + 3 O2(g) = 6 SO3(g) None of the above reactions have Kc = Kp.
Calculate S^0 of NH_3(g) for the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) using the following data: Delta G_f^0 of NH_3(g) = - 16 kJ/mol Delta H_f^0 of NH_3(g) = - 45.9 kJ/mol S^0 of H_2(g) = 131 J/mol. K S^0 of N_2(g) = 191.5 J/mol. K
a. write the equilibrium expression and for the balanced reaction: 2 SO_3 (g) leftarrow and rightarrow 2 SO_2 (g) + O_2 (g). b. Given the following information: [SO_3] = 0.0255M, [SO_2] = 1.08M, and [O_2] = 1.45M at equilibrium calculate the equilibrium constant K. The oxidation of ammonia is a reversible exothermic reaction that proceeds as follows: 4 NH_3(g) + 5 O_2(g) leftarrow rightarrow 4 NO(g) + 6 H_2O(g) + heat For each situation described in the table, indicate the...
Calculate the enthalpy of formation of SO_2(g) from the standard enthalpy changes of the following reactions: SO_2(g) + O_2(g) rightarrow 2 SO_3(g) Delta H degree _r times n = - 196 kJ S(s) + 3 O_2(g) rightarrow 2 SO_3(g) Delta H degree _r times n = - 790 kJ S(s) + O_2(g) rightarrow SO_2(g) Delta H degree _r times n = Number _______ kJ
K_p for NH_3 at 25 degree C N_2 (g) + 3 H_2(g) irreversible 2 NH_3 (g), Delta G degree = -31.0 kJ consider the galvanic cell that uses the reaction 2 Ag^+ (aq) plus Cu(s) rightarrow Cu^2+ (aq) + 2Ag (s) clearly sketch the experimental set-up, write down the anode and cathode half- give the shorthand notation for the cell For the following cell, write a balanced equation for the cell reaction and calc Delta G degree C: Pt(s) |H_2(1.0...
Question 11 In which of the following reactions will Kc = Kp? H2(g) + 12(g)=2 HI(g) CH4(g) + H2O(g) = CO(g) + 3H2(g) N204(8)=2NO2(g) ON2(g) + 3 Cl2(g) = 2 NCl3(g) O CO(g) + 2 H2(g)=CH3OH(g) < Previous
Consider the reaction below at 850 K: 2SO 2 (g)+O 2 (g)⇌2SO 3 (g) Kc=15 Now lets think about how the reaction will proceed under the following sets of starting conditions. In each case predict if the reaction will proceed: \textbf{forwards,}forwards, or \textbf{backwards}backwards. [SO2] = 0.15 M, [O_2][O2] = 0.68 M, [SO_3][SO3] = 0.36 M The value of Q is The reaction will proceed [SO_2][SO 2 ] = 0.18 M, [O_2][O 2 ] = 0.10...
Classify the following reactions as either: combination, decomposition, combustion, precipitation (metathesis) or redox reactions. C(s) + 4 HNO_3 (aq) rightarrow 4 NO_2 (g) + 2 H_2 O (I) + CO_2 (g) HCI (aq) + NH_3 (aq) rightarrow NH_4 CI(aq) 2HI (g) rightarrow H_2 (g) + I_2 (g) Cu(NO_3)_2 9aq) + Na_2 S (aq) rightarrow CuS(s) + 2 NaNO_3 (aq) Zn(s) + 2 AgNO_3 (aq) rightarrow Zn(NO_3)_2 (aq) + 2 Ag(s) H_2 SO_3 (aq) + 2 KOH(aq) rightarrow K_2 SO_3 (aq)...