QuestionJuly 17, 2025

Using Delta G calculate the value of the thermodynamic equilibrium constant K for: H_(2)(g)+Br_(2)(l)- -gt 2HBr(g)

Using Delta G calculate the value of the thermodynamic equilibrium constant K for: H_(2)(g)+Br_(2)(l)- -gt 2HBr(g)
Using Delta G calculate the value of the thermodynamic equilibrium constant K for: H_(2)(g)+Br_(2)(l)- -gt 2HBr(g)

Solution
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Answer

K = e^{-\Delta G / (RT)} Explanation 1. Identify the relationship between \Delta G and K The relationship is given by the formula: **\Delta G = -RT \ln K**, where R is the gas constant and T is the temperature in Kelvin. 2. Rearrange the formula to solve for K Rearrange to get: **K = e^{-\Delta G / (RT)}**. 3. Substitute known values Use R = 8.314 \, \text{J/mol K} and substitute the given \Delta G and T into the equation to calculate K.

Explanation

1. Identify the relationship between $\Delta G$ and $K$<br /> The relationship is given by the formula: **$\Delta G = -RT \ln K$**, where $R$ is the gas constant and $T$ is the temperature in Kelvin.<br /><br />2. Rearrange the formula to solve for $K$<br /> Rearrange to get: **$K = e^{-\Delta G / (RT)}$**.<br /><br />3. Substitute known values<br /> Use $R = 8.314 \, \text{J/mol K}$ and substitute the given $\Delta G$ and $T$ into the equation to calculate $K$.
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