Use a thermodynamic table to find the equilibrium constant for the nonideal-gas reaction 2HC1(g) H2 (g)...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) ---------->2HI(g) 1) Calculate the equilibrium concentrations of reactants and product when 0.309 moles of H2 and 0.309 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M? [I2] = M? [HI] = M? 2.The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K: PCl5(g)------->PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a...
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. H2(g) + Cl2(g)—>2HCI(g) K=
For the reaction H2(g) +
Cl2(g) 2 HCl(g), the
equilibrium constant K at 800oC is 4.35 x
104.
Hydrogen and chlorine, each at a partial pressure of 0.700 bar,
are placed in a vessel at 800oC and allowed to
equilibrate. Find the final partial pressures of all three gases in
this reaction.
p(H2) = bar
p(Cl2) =
. bar
p(HCl) =
bar
1)
2)
3)
4)
The equilibrium constant for the gas phase reaction 2803 (g) = 2802 (g) + O2 (g) is Keg = 7.1 x 102 at 999 K. At equilibrium,_ O only reactants are present O roughly equal amounts of products and reactants are present products predominate only products are present reactants predominate QUESTION 20 The rate law of a reaction is rate = k[X]-. The units of the rate constant are O mol L-15-2 OL mol-15-1 O mol2...
Given the thermodynamic data below, calculate the value of the
equilibrium constant for the reaction shown at 25.0ºC
H₂ (g) + I₂ (g) ⇄ 2 HI (g)
Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown at 25.0°C H2(g) + 12 (g) = 2 HI(g) AH° = -9.48 kJ AS° = +21.79 J/K K= at 25.0°C Check
Calculate the equilibrium constant of the reaction CO(g) + H2(g) ⇌ H2CO(g) given that for the production of liquid formaldehyde ΔrG< = +28.95 kJ mol−1 at 298 K and that the vapour pressure of formaldehyde is 1500 Torr at that temperature.
For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35 x 10^4. Hydrogen at a partial pressure of 0.700 bar and chlorine at a partial pressure of 0.500 bar are placed in a vessel at 800oC and allowed to equilibrate. Find the final partial pressures of all three gases in this reaction in bar
(1). The equilibrium constant, Kp, for the following reaction is 1.80×10-2 at 698K. 2HI(g) =H2(g) + I2(g) If an equilibrium mixture of the three gases in a 15.5 L container at 698K contains HI at a pressure of 0.399 atm and H2 at a pressure of 0.562 atm, the equilibrium partial pressure of I2 is atm. (2). Consider the following reaction: PCl5(g) =PCl3(g) + Cl2(g) If 1.17×10-3 moles of PCl5, 0.217 moles of PCl3, and 0.351 moles of Cl2 are at...
Consider the reaction given below.
H2(g) + F2(g)
2 HF(g)
(a) Using thermodynamic data from the course website, calculate
G° at 298 K.
kJ
(b) Calculate G at 298 K if the reaction mixture
consists of 5.1 atm of H2, 4.8 atm of F2, and
0.19 atm of HF.
kJ
Consider the reaction given below.
H2(g) + F2(g)
2 HF(g)
(a) Using thermodynamic data from the course website, calculate
G° at 298 K.
____ kJ
(b) Calculate G at 298 K if the reaction mixture
consists of 8.3 atm of H2, 3.0 atm of F2, and
0.26 atm of HF.
____ kJ