Question

In: Chemistry

Kp = 6.5 × 104 at 308 K for the following reaction: 2 NO (g) +...

Kp = 6.5 × 104 at 308 K for the following reaction:

2 NO (g) + Cl2(g) ⇌ 2 NOCl(g)

At equilibrium,  PNO = 0.35 atm and PCl2 = 0.10 atm

What is the equilibrium partial pressure of NOCl(g)?

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago
Next > < Previous

Related Solutions

1) At a certain temperature, 322 K, Kp for the reaction, Cl2(g) <=> 2 Cl(g), is...
1) At a certain temperature, 322 K, Kp for the reaction, Cl2(g) <=> 2 Cl(g), is 7.82 x 10-60. Calculate the value of ΔGo in kJ for the reaction at this temperature. 2) The equilibrium constant for the reaction, 2 Fe3+(aq) + Hg22+(aq) <=> 2 Fe2+(aq) + 2 Hg2+(aq) is 9.1 x 10-6(aq) at 298 K. Calculate ΔG in J when {Fe3+(aq)} = 0.375 {Hg22+(aq)} = 0.051 {Fe2+(aq)} = 0.021 {Hg2+(aq)} = 0.06
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) Kp=2.26×104 at 25 ∘C. Calculate ΔGrxn for the reaction at 25...
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) Kp=2.26×104 at 25 ∘C. Calculate ΔGrxn for the reaction at 25 ∘C under each of the following conditions. - standard conditions - at equilibrium - PCH3OH= 1.4 atm ; PCO=PH2= 1.5×10−2 atm
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) Kp=2.26×104 at 25 ∘C. Calculate ΔGrxn for the reaction at 25...
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) Kp=2.26×104 at 25 ∘C. Calculate ΔGrxn for the reaction at 25 ∘C under each of the following conditions. A) Standard conditions B) At equilibrium C) PCH3OH= 1.5 atm ; PCO=PH2= 1.5×10−2 atm
The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP =...
The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP = 0.032 at a particular temperature. At that temperature, a vessel is filled with 0.040 atm of N2 (g), 0.040 atm of O2 (g) and 0.043 atm of NO (g). What is the pressure of NO (g) at equilibrium?
The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K: PCl3(g) + Cl2(g)...
The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K: PCl3(g) + Cl2(g) <----->PCl5(g) Calculate the equilibrium partial pressures of all species when PCl3 and Cl2, each at an intitial partial pressure of 1.56 atm, are introduced into an evacuated vessel at 500 K. PPCl3 = atm PCl2 = atm PPCl5 = atm
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g)...
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium partial pressures of all species when CO and Cl2, each at an intitial partial pressure of 1.65 atm, are introduced into an evacuated vessel at 600 K. PCO = ______ atm PCl2= _______ atm PCOCl2 = _______ atm
The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K: PCl3(g) + Cl2(g)...
The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K: PCl3(g) + Cl2(g) <<<----->>PCl5(g) Calculate the equilibrium partial pressures of all species when PCl3 and Cl2, each at an intitial partial pressure of 1.01 atm, are introduced into an evacuated vessel at 500 K. PPCl3 = atm PCl2 = atm PPCl5 = atm
Consider the following reaction where Kp = 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) If...
Consider the following reaction where Kp = 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) If the three gases are mixed in a rigid container at 600 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: 1. A reaction will occur in which COCl2(g) is produced 2. Kp will decrease. 3. A reaction will occur in which CO is produced. 4. Q...
1. The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) <--->CH4(g)...
1. The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) <--->CH4(g) + CCl4(g) Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.865 atm at 350 K. PCH2Cl2 =____ atm PCH4 =____ atm PCCl4 =____ atm 2. The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K: NH4I(s) <----> NH3(g) + HI(g) Calculate the equilibrium partial pressure of HI when 0.413...
1)The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) The equilibrium...
1)The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <------ ------> PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.14 atm at 500 K. PPCl5 = atm PPCl3 = atm PCl2 = atm 2) The equilibrium constant, Kp, for the following reaction is 55.6 at 698...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT