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...
1. The equilibrium constant, Kc, for the following reaction is 42.2 at 288 K. 2CH2Cl2(g) <-----> CH4(g) + CCl4(g) When a sufficiently large sample of CH2Cl2(g) is introduced into an evacuated vessel at 288 K, the equilibrium concentration of CCl4(g) is found to be 0.140 M. Calculate the concentration of CH2Cl2 in the equilibrium mixture. _____ M 2. A student ran the following reaction in the laboratory at 295 K: 2CH2Cl2(g) <-------> CH4(g) + CCl4(g) When she introduced 8.46×10-2 moles...