What would happen to the calculated molar volume of CO2 if a student warmed the

Question

What would happen to the calculated molar volume of CO2 if a student warmed the flask with a price of dry ice in it above room temperature with their hands? Would it cause the calculated molar volume to be too low, too high or unaffected? Briefly explain please
What would happen to the calculated molar volume of CO2 if a student warmed the flask with a price of dry ice in it above room temperature with their hands? Would it cause the calculated molar volume to be too low, too high or unaffected? Briefly explain please
What would happen to the calculated molar volume of CO2 if a student warmed the flask with a price of dry ice in it above room temperature with their hands? Would it cause the calculated molar volume to be too low, too high or unaffected? Briefly explain please

Explanation / Answer

Dry ice is solid carbon dioxide, with the formula CO2. The temperature of dry ice in its transition from an ordinary state to a gaseous state is -78.5 oC.

When a piece of dry ice is added to the flask, that is you have added some quantity of CO2 to the flask. When you warm the flak above room tempperature, the solid CO2 will convert to gas CO2. That is moles of CO2 has increased.

And hence, the calculated molar volume will be equal to the original molar volume of CO2 in the flask plus the molar volume of CO2 (from the dry ice, that is solid CO2, converting to gaseous phase).

Hence, the the calculated molar volume would be high than the original molar volume.

Hence the total molar

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