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11 Dec 2019

What is Δn for the following equation in relating Kc to Kp?

N2(g) + 3 F 2(g) ↔ 2 NF 3(g)

What is Δn for the following equation in relating Kc to Kp?

N2(g) + 3 F 2(g) ↔ 2 NF 3(g)

1
-2
4
-4
2

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Related questions

What is Δn for the following equation in relating Kc to Kp?

2K(s) + 2H2O(l) ⇋ 2 KOH(aq) + H2(g)
A. -4

B. 3

C. 1

D.-2

E. 0

The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation

Kp=Kc(RT)Δn

where R=0.08206 L⋠atm/(K⋠mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction

N2(g)+3H2(g)⇌2NH3(g)

for which Δn=2−(1+3)=−2.

For the reaction

3A(g)+3B(g)⇌C(g)

Kc = 78.0 at a temperature of 283 ∘C .

Calculate the value of Kp.

Part 2

For the reaction

X(g)+2Y(g)⇌3Z(g)

Kp = 3.45×10−2 at a temperature of 367 ∘C .

Calculate the value of Kc.

The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋠atm/(K⋠mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2. A. For the reaction 3A(g)+3B(g)⇌C(g) Kc = 94.0 at a temperature of 333 ∘C . Calculate the value of Kp. B: For the reaction X(g)+2Y(g)⇌3Z(g) Kp = 3.39×10−2 at a temperature of 375 ∘C . Calculate the value of Kc.

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