Densities of diamond and graphite are 3.5 and 2.3g/cm^3 respectively. Increase of the pressure on equillbrium cdiamond gives c graphite
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If there was a greater pressure, then this would lead to a reduction in volume; normally, an equilibrium shifts to the side with less mols of gas, or less volume. Since graphite has a lower density, equilibrium will shift to the left if the pressured it increased. Therefore, it will shift to the right, diamond, if the pressure is decreased. So low pressure for this one.
For the temperature, this is an endothermic reaction. Therefore, heat is used in the reactants to produce the products. When heat is added to the reaction (high temperature), it's added to the reactants. This causes an offset of the equilibrium, and to correct this, the equilibrium shifts to the right to use up added heat, giving more diamond. So a high temperature would yield more diamond.
Best Answer
If there was a greater pressure, then this would lead to a reduction in volume; normally, an equilibrium shifts to the side with less mols of gas, or less volume. Since graphite has a lower density, equilibrium will shift to the left if the pressured it increased. Therefore, it will shift to the right, diamond, if the pressure is decreased. So low pressure for this one.
For the temperature, this is an endothermic reaction. Therefore, heat is used in the reactants to produce the products. When heat is added to the reaction (high temperature), it's added to the reactants. This causes an offset of the equilibrium, and to correct this, the equilibrium shifts to the right to use up added heat, giving more diamond. So a high temperature would yield more diamond.
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