questions 1 & 2 1. The following reaction occurs at 419 K. kpke (RT 3X(g) +...
The equilibrium constant, Kc, for the following reaction is 2.02×10-2 at 745 K. 2HI(g) <--> H2(g) + I2(g) Calculate Kc at this temperature for: H2(g) + I2(g) <--> 2HI(g) Kc =
The equilibrium constant, Kc, for the following reaction is 1.68×10-2 at 672 K. 2HI(g) <---> H2(g) + I2(g) Calculate Kc at this temperature for: H2(g) + I2(g) <---> 2HI(g) Kc =
Consider the chemical reaction below at a given temperature and at equilibrium: H2(g) +12(g) = 2HI(g) Kc = 53.3 If 0.800 mol of H2 and 0.800 mol of 12 are placed in a 1.00L container and allowed to react, what is the [HI] when the reaction reaches equilibrium? [HIN In the expression for K N- (H2] [12]' The equilibrium concentrations can be expressed as follows: NOTE: This is NOT asking for the concentrations you solve for this is literally asking...
The equilibrium constant, Kc, for the following reaction is 2.02×10-2 at 745 K. 2HI(g) <---> H2(g) + I2(g) Calculate Kc at this temperature for the following reaction: 1/2H2(g) + 1/2I2(g) <---> HI(g) Kc =
1- At a certain temperature, 0.820 mol of SO3 is placed in a 2.50-L container. 2SO3(g)---->2SO2(g)+O2(g) At equilibrium, 0.120 mol of O2 is present. Calculate Kc. 2- At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g)----->2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium? 3-Carbon disulfide is prepared by heating sulfur and charcoal....
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) +12(g) = 2 HI(g) Kc = 53.3 At this temperature, 0.500 mol H, and 0.500 moll, were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI] =
At a certain temperature, the equilibrium constant, Ke, for this reaction is 53.3. H,(g) +12(R) 근 2H1(R) K, 53.3 At this temperature, 0.700 mol of H2 and 0.700 mol of I2 were placed in a 1.00-L container to react. What concentration of Hl is present at equilibrium? Number
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H,(g) +1,(g) = 2 HI(g) K. = 53.3 At this temperature, 0.300 mol H, and 0.300 mol I, were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI] =
What is the relationship between K, and K, for the reaction, 2ICI(g)#12(9) + C12 Cl2(g)? º Kp = K (RT)-1 O Kp = Kc(RT) ° Kp = K (RT)2 OKp = K.
Consider the following equilibrium with a Kc = 55.6 at a temperature of 698 K. H2(g) + I2(g) <--> 2HI(g) ΔH0 = + 26.5 kJ / mol If the initial concentrations were [H2] = 0.12 M; [I2] = 0.041 M; and [HI] = 2.6 M. Is the system at equilibrium, and if not, in which direction must it shift to establish equilibrium? Justify your answer. At the same 698 K, 0.50 mol of H2 and 0.88 mol of I2 are...