The following reaction has an equilibrium constant K = 4.00×10−3. 2HCN

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The following reaction has an equilibrium constant K = 4.00×10−3. 2HCN(g) ⇌ H2(g) + C2N2(g) Some amounts of HCN and H2 are introduced into a reaction vessel, and the system is allowed to come to equilibrium. The resulting equilibrium concentrations are [HCN] = 0.970 M, and [C2N2] = 0.042 M. Calculate the equilibrium concentration of H2. Answer in molarity to at least three significant figures.

The following reaction has an equilibrium constant K = 4.00×10−3. 2HCN(g) ⇌ H2(g) + C2N2(g) Some amounts of HCN and H2 are introduced into a reaction vessel, and the system is allowed to come to equilibrium. The resulting equilibrium concentrations are [HCN] = 0.970 M, and [C2N2] = 0.042 M. Calculate the equilibrium concentration of H2. Answer in molarity to at least three significant figures.

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The following reaction has an equilibrium constant

K = 4.00 \times 10^{- 3}

.

2 H C N (g) ⇌ H_{2} (g) + C_{2} N_{2} (g)

Some amounts of

H C N

and

H_{2}

are introduced into a reaction vessel, and the system is allowed to come to equilibrium. The resulting equilbrium concentrations are

[H C N] = 0.970

M

, and

[C_{2} N_{2}] = 0.042 M

. Calculate the equilibrium concentration of

H_{2}

. Answer in molarity to at least three significant figures.

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