Calculate the value of the equilibrium constant, K, for the reaction Q(g) + X(g) = 2...
Calculate the value of the equilibrium constant, Kc , for the reaction Q(g) + X(g) = 2 M(g) + N(g) given that M(g) = 2(g) 6 R(g) = 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kci = 3.42 Kc2 = 0.496 Kc3 = 11.4 Kc =
Calculate the value of the equilibrium constant, ?c , for the reaction Q(g)+X(g)↽−−⇀2M(g)+N(g) Q ( g ) + X ( g ) ↽ − − ⇀ 2 M ( g ) + N ( g ) given that M(g)↽−−⇀Z(g)6R(g)↽−−⇀2N(g)+4Z(g)3X(g)+3Q(g)↽−−⇀9R(g)?c1=3.21?c2=0.495?c3=13.4 M ( g ) ↽ − − ⇀ Z ( g ) K c 1 =3.21 6R ( g ) ↽ − − ⇀ 2N ( g ) +4Z ( g ) K c 2 =0.495 3X ( g ) +3Q...
Calculate the value of the equilibrium constant, ?ccc , for the reactionQ(g)+X(g)↽−−⇀2M(g)+N(g)Q(g)+X(g)↽−−⇀2M(g)+N(g)given thatM(g)↽−−⇀Z(g)6R(g)↽−−⇀2N(g)+4Z(g)3X(g)+3Q(g)↽−−⇀9R(g)?c1=3.05?c2=0.443?c3=11.5?cKc= _________
Calculate the value of the equilibrium constant, ?cKc , for the reactionQ(g)+X(g)↽−−⇀2M(g)+N(g)Q(g)+X(g)↽−−⇀2M(g)+N(g)given thatM(g)↽−−⇀Z(g)6R(g)↽−−⇀2N(g)+4Z(g)3X(g)+3Q(g)↽−−⇀9R(g)?c1=3.05?c2=0.443?c3=11.5?c=Kc= _________
Calculate the value of the equilibrium constant, ?c , for the reaction Q(g)+X(g)↽−−⇀2M(g)+N(g) given that M(g)↽−−⇀Z(g)6R(g)↽−−⇀2N(g)+4Z(g)3X(g)+3Q(g)↽−−⇀9R(g)?c1=3.85?c2=0.459?c3=14.7
Calculate the value of the equilibrium constant, ?c , for the reaction Q(g)+X(g)↽−−⇀2M(g)+N(g) given that M(g)↽−−⇀Z(g)6R(g)↽−−⇀2N(g)+4Z(g)3X(g)+3Q(g)↽−−⇀9R(g)?c1=3.71?c2=0.595?c3=14.2
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) >>CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.327 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. [CH2Cl2] = M [CH4] = M [CCl4] = M The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) >>CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.275 moles of COCl2(g) are...
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) = PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.249 moles of PCl3 and 0.249 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = M [Cl2] = M [PCl5] = M The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) = H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and...
12. The equilibrium constant for the reaction: SO2(g) + O2(g)so,(g) is Kc # 1.3 x 10, What is the equilibrium constant for the reaction: 2S0,(g)O,(g)+ 2S02(g) 13. For the following reaction, Kc (@ 500 K) 1.0 x 10 2 SO-(g) + 02(g) 2 SO,(g). What is the value of Kp for this reaction at 500 K? (3 Pts.)