Consider the reaction. PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=0.0420 PCl 5 ( g ) ↽ − − ⇀ PCl 3 ( g ) + Cl 2 ( g ) K c = 0.0420 The concentrations of the products at equilibrium are [PCl3]=0.270 M [ PCl 3 ] = 0.270 M and [Cl2]=0.180 M [ Cl 2 ] = 0.180 M . What is the concentration of the reactant, PCl5 PCl 5 , at equilibrium? [PCl5]= [ PCl 5 ] =
Consider the reaction. PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=0.0420 PCl 5 ( g ) ↽ − − ⇀ PCl 3 (...
Consider the reaction. PCl5(g)−⇀↽−PCl3(g)+Cl2(g)Kc=0.0420 The concentrations of the products at equilibrium are [PCl3]=0.180 M and [Cl2]=0.280 M. What is the concentration of the reactant, PCl5, at equilibrium?
Consider the reaction. PCl5(g)↽−−⇀PCl3(g)+Cl2(g)?c=0.0420 The concentrations of the products at equilibrium are [PCl3]=0.120 M and [Cl2]=0.150 M. What is the concentration of the reactant, PCl5, at equilibrium?
Consider the reaction. PCl (g)PC3(g) + Cl2(g) Ke = 0.0420 The concentrations of the products at equilibrium are [PCl3] = 0.200 M and [Cl2] = 0.190 M. What is the concentration of the reactant, PCI5, at equilibrium? PCI5 M
Consider the reaction: PCl5 (g) ⇔ PCl3 (g) + Cl2 (g) The initial concentration of PCl5 is 0.40 M and the equilibrium concentration of PCl3 is 0.33 M. Calculate the equilibrium constant Kc.
Consider the reaction. PCI; (g) = PCI,(g) + Cl2(g) Kc = 0.0420 The concentrations of the products at equilibrium are [PC13] = 0.160 M and [Cl2] = 0.160 M. What is the concentration of the reactant, PCs, at equilibrium? [PCI31= C [PCIS] = M
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...
Consider the reversible reaction. PCl5↽−−⇀PCl3+Cl2PCl5↽−−⇀PCl3+Cl2 Are the concentrations of phosphorus pentachloride, PCl5,PCl5, and phosphosphorus trichloride, PCl3,PCl3, constant or changing at equilibrium? The concentration of PCl5PCl5 is constant, and the concentration of PCl3PCl3 is changing at equilibrium. The concentration of PCl5PCl5 is changing, and the concentration of PCl3PCl3 is constant at equilibrium. The concentrations of both PCl5PCl5 and PCl3PCl3 are constant at equilibrium. The concentrations of both PCl5PCl5 and PCl3PCl3 are changing at equilibrium. which one is correct please explain
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 0.253 moles of PCl3 and 0.253 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 83.3 at 500 K. PCl3(g) + Cl2(g) -----> PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.504 moles of PCl3 and 0.504 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 83.3 at 500 K. PCl3(g) + Cl2(g) PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.366 moles of PCl3 and 0.366 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = ____M [Cl2] = _____M [PCl5] = ____M