Advanced Higher Chemistry
Can someone help with this equilibrium questions please!!
The industrial production of ‘freon’, CCl2F2(g), is represented by the following equation.
1 mol of CCl4(g) and 2 mol of HF(g) are introduced into an empty reaction chamber. When equilibrium is established, it is found that 0.75 mol of ‘freon’ has been formed. Calculate the equilibrium constant, K, for the reaction under these conditions.(2)
The industrial production of ‘freon’, CCl2F2(g), is represented by the following equation.
1 mol of CCl4(g) and 2 mol of HF(g) are introduced into an empty reaction chamber. When equilibrium is established, it is found that 0.75 mol of ‘freon’ has been formed. Calculate the equilibrium constant, K, for the reaction under these conditions.(2)
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Im confused about this chemistry question, why does it form these productsTrending
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