1.If Kp = 845 for the reaction below at 310.0 K, then what is the value of Kc?(R = 0.0821 L･atm/mol･K.) 2 A (g) + B (s) ⇌ 2 C (s) + D (g) 2.A reaction vessel initially contains only 3.5 atm of N₂O₄. When the system reaches equilibrium according to the reaction below, there is 1.7 atm of NO₂ in the vessel. What is Kp for this reaction? 2 NO₂ (g) ⇌ N₂O₄ (g) 3.A solution is made initially with 0.440 M HIO₃ (Kc = 0.170). Once the equilibrium below is established, what
1.If Kp = 845 for the reaction below at 310.0 K, then what is the value of Kc?(R = 0.0821 L･atm/mol･K.) 2 A (g) + B (s) ⇌ 2 C (s) + D (g)
2.A reaction vessel initially contains only 3.5 atm of N₂O₄. When the system reaches equilibrium according to the reaction below, there is 1.7 atm of NO₂ in the vessel. What is Kp for this reaction? 2 NO₂ (g) ⇌ N₂O₄ (g)
3.A solution is made initially with 0.440 M HIO₃ (Kc = 0.170). Once the equilibrium below is established, what is the equilibrium concentration of H⁺ ions? HIO₃ (aq) ⇌ H+ (aq) + IO₃⁻ (aq)
4.An empty steel container is filled with 0.0580 atm of HF. The system is allowed to reach equilibrium. If Kp = 2.76 for the reaction below, what is the equilibrium partial pressure of H₂? 2 HF (g) ⇌ H₂ (g) + F₂ (g)
(1) By help of Following formula we can calculate the value of Kc -
Kp = Kc (RT)∆n
Here , Kp is Equilibrium constant for Gaseous Reaction (845)
Kc is Equilibrium constant for concentration
R is gas constant = 0.0821 L atm/mol K
T is temperature= 310 K
∆n is number of moles changed in Reaction 2 A (g) + B (s) ⇌ 2 C (s) + D (g) , it is 1-2 = -1
Then,
845 = Kc (0.0821×310)-1
Kc = 845 × (0.0821 × 310 ) = 21506.095
Kc = 21506.1
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