A sample consisting of CO₂(g) and CO₂(s) at equilibrium at -78°C and 1 atm pressure is heated to -30°C, and the pressure is increased to 8 atm. Based on the phase diagram below, what will happen? A) At equilibrium, only CO₂(g) will be present. B) The melting point of the CO₂(s) will decrease. C) At equilibrium, CO₂(g) and CO₂(l) will be present. D) All the CO₂ will be converted to CO₂(l). E) none of these

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The Answer of A sample consisting of CO₂(g) and CO₂(s) at equilibrium at -78°C and 1 atm pressure is heated to -30°C, and the pressure is increased to 8 atm. Based on the phase diagram below, what will happen? A) At equilibrium, only CO₂(g) will be present. B) The melting point of the CO₂(s) will decrease. C) At equilibrium, CO₂(g) and CO₂(l) will be present. D) All the CO₂ will be converted to CO₂(l). E) none of these

A Sample Consisting of CO2(g) and CO2(s) at Equilibrium at -78°C

A Sample Consisting of CO₂(g) and CO₂(s) at Equilibrium at -78°C