Indicate whether the following reaction contains mostly reactants, mostly products, or both reactants and products at equilibrium: $2HF(g) \rightleftharpoons H_2(g) + F_2(g)$, $K_c = 1.0 \times 10^{-95}$
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0 \times 10^{-95}$. This value is extremely small. Show more…
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In a reaction like this, how would we know that the change is negative in the reactants while positive in the products or vice versa?
David C.
Hydrogen fluoride decomposes according to the following equation: $$ 2 \mathrm{HF}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) $$ The value of $K_{c}$ at room temperature is $1.0 \times 10^{-95} .$ From the magnitude of $K_{c}$, do you think the decomposition occurs to any great extent at room temperature? If an equilibrium mixture in a 1.0-L vessel contains $1.0 \mathrm{~mol} \mathrm{HF}$, what is the amount of $\mathrm{H}_{2}$ formed? Does this result agree with what you expect from the magnitude of $K_{c}$ ?
Hydrogen fluoride decomposes according to the following equation: $$ 2 \mathrm{HF}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) $$ The value of $K_{c}$ at room temperature is $1.0 \times 10^{-95}$. From the magnitude of $K_{c}$, do you think the decomposition occurs to any great extent at room temperature? If an equilibrium mixture in a 1.0 - $\mathrm{L}$ vessel contains $1.0 \mathrm{~mol} \mathrm{HF}$, what is the amount of $\mathrm{H}_{2}$ formed? Does this result agree with what you expect from the magnitude of $K_{c} ?$
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