For N2g - 3H2g - 2NH3g - heat- the rate constant is-

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Heat of Reaction

For N2g + 3...

Question

For $N_{2} (g) + 3 H_{2} (g) \Leftrightarrow 2 N H_{3} (g) + h e a t$ , the rate constant is:

K_{p} = K_{c}

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K_{p} = K_{c} \times (R T)

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K_{p} = K_{c} \times (R T)^{- 2}

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K_{p} = K_{c} \times (R T)^{- 1}

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Solution

The correct option is C $K_{p} = K_{c} \times (R T)^{- 2}$
The relationship between $K_{p}$ and $K_{c}$ is $K_{p} = K_{c} (R T)^{Δ n}$ .
For the reaction $N_{2} (g) + 3 H_{2} (g) \Leftrightarrow 2 N H_{3} (g) + h e a t$ , the value of $Δ n$ is $2 - (1 + 3) = - 2$ .
Substitute this value in the above expression.
$K_{p} = K_{c} (R T)^{Δ n} = K_{c} (R T)^{- 2}$ .

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Similar questions

Q. Assertion :

K_{p} = K_{c}

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are interrelated by the equation

K_{p} = K_{c} {(R T)}^{Δ n}

Q. The value of

\frac{K_{p}}{K_{c}}

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are, respectively:

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

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[A t 300 K, R T = 24.62 d m^{3} a t m m o l^{- 1}]

For a general reaction aA(g) + bB(g) $⇋$ cC(g)+ dD(g), what is the relationship between the equilibrium constants $K_{c}$ and $K_{p}$ ? [assume $Δ$ n = $μ$ = (c + d) - (a+b) ]\)

Q. The equilibrium constant

K_{c}

for the reaction

N_{2 (g)} + 3 H_{2} ⇌ {2 N H}_{3 (g)}

0.286

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. Calculate

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Q. Drive the following relation:

K p = K c (R T)^{n}

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For N2(g)+3H2(g)⇔2NH3(g)+heat, the rate constant is:

The correct option is C Kp=Kc×(RT)−2The relationship between Kp and Kc is Kp=Kc(RT)Δn.For the reaction N2(g)+3H2(g)⇔2NH3(g)+heat, the value of Δn is 2−(1+3)=−2.Substitute this value in the above expression.Kp=Kc(RT)Δn=Kc(RT)−2.

For $N_{2} (g) + 3 H_{2} (g) \Leftrightarrow 2 N H_{3} (g) + h e a t$ , the rate constant is: