1)
Kc = [HI]^2 / [H2][I2]
Put units:
Kc = [mol/L]^2 / [mol/L]*[mol/L]
= (mol^2/L^2) / (mol^2/L^2)
= 1
Answer: D
2)
Kc = [NH3]^2 / [H2]^3[N2]
Put units:
Kc = [mol/L]^2 / [mol/L]^3[mol/L]
= (mol^2/L^2) / (mol^4/L^4)
= mol^-2.L^2
Answer: B
3)
T = 700 K
Δ n = number of gaseous molecule in product - number of gaseous molecule in reactant
Δ n = 0
use:
Kp= Kc (RT)^Δ n
Kp = 0.11*(0.08206*700.0)^(0)
Kp = 0.11
Answer: B
Only 1 question at a time please
Choosa the correct answer : 1. K unit in the balanced reaction : H2 +12 ->...
________________________________________________________________ ________________________________________________________________________ The equilibrium-constant expression for a gas reaction is [N, H4] [N][H,12 Choose the balanced chemical equation corresponding to this expression. N2(g) + 2H2 (9) = N2H (9) ON, H. (g) = N2(g) + 2H2 (9) N2(9) + H2(9) N2H4(9) 2N2 (9) + 4H2(g) = 2N, H4 (9) Iodine and bromine react to give iodine monobromide, IBr. 12 (9) + Br2(g) = 21Br(9) What is the equilibrium composition of a mixture at 126°C that initially contained 1.30 x 10...
Consider the reaction: N2(g) + 3 H2(g) « 2 NH3(g) a. Write the expression for the equilibrium constant, K, for this reaction. b. An equilibrium misture of N2, H2, and NH3 at 300°C is analyzed, and it is found that: [N2] = 0.25 mol/L, [H2] = 0.15 mo/L, and [NH3] = 0.090 mol/L. Find K at 300°C for this reaction.
The following reaction was carried out in a 3.75 L reaction vessel at 1100 K: C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 8.50 mol of C, 12.7 mol of H2O, 4.00 mol of CO, and 6.20 mol of H2, what is the reaction quotient Q? Enter the reaction quotient numerically. Q = Consider the reaction CO(g)+NH3(g)⇌HCONH2(g), Kc=0.810 If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00...
Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + CO2(g) ⇌ H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.72 mol H2 and 0.72 mol CO2 are injected into a 4.5−L flask. Calculate the concentration of each species at equilibrium. Equilibrium concentration of H2: M Equilibrium concentration of CO2: M Equilibrium concentration of H2O: M Equilibrium concentration of CO: M
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a certain temperature, the equilibrium concentrations are [NO]-0.31 M [H2]-0.16 M [N2] 0.082 M and [H:0]-4.64 M (a) Write the equilibrium expression for the reaction. (b) Determine the value of the equilibrium constant 2. The equilibrium constant Kc for the following reaction is 150.7 at 1 15°C: 12 (g) + Br2 (g) ←→ 2 IBr(g) 2.00 moles of each gas (l2, Br: and IBr) are...
For the unbalanced reaction H2(g)+NO(g) ---> H2O(g)+N2(g): the initial concentrations are 5.25 M H2, 9.00 M NO, and no H2O or N2. At equilibrium, [N2] = 1.75 M. A) Balance the equation using lowest-whole-number coefficients. Be sure to include states of matter in your equation. B) Calculate the value of K under the reaction conditions at equilibrium.
The equilibrium constant K for the reaction N2 + 3H22NH, is 0.159 at 450°C. Calculate the equilibrium composition when 2.50 mol N2 is mixed with 7.50 mol H2 in a 5.00 L vessel. [N] - M [H2] M (NH3) M Submit Answer Try Another Version 6 Item attempts remaining
1. Solve for K under the following conditions with the following reaction: PbO (s) + 2H + (aq) ⇌ Pb2+ (aq) + 2H2O (l) PbO (s) = 8.67 g [H + ] = 3.43 M [Pb 2+ ] = 0.311 M H2O (l) = 5.02 M Find K 2. H2 (g) + I2 (s) ⇌ 2 HI (g) 0.162 atm H2 (g), 8.012 g I2 (s), 1.449 atm HI (g) Calculate the pressures of H2 and HI at equilibrium.
A.) Calculate K for a reaction that has ∆H0 = -5.65 KJ/mol and ∆S0 = 43.75 J/mol K at 298.15 K. B.) Calculate ∆S0 for a reaction that has ∆H0 = 11.36 KJ/mol and K = 0.000376 at 298.15 K. Report your answer in J/mol K C.) Consider the reaction below. 2 NH3 ⇋ N2 + 3 H2 When 1.45 M NH3 wis allowed to decompose until equilibrium has been achieved, 0.87 M NH3 remains. If this reaction has ∆S0 =...
The following reaction was carried out in a 4.00 L reaction vessel at 1100 K: C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 5.50 mol of C, 16.0 mol of H2O, 3.40 mol of CO, and 7.00 mol of H2, what is the reaction quotient Q?