At normal atmospheric pressure of 1.00 atm, solid carbon dioxide (‘dry ice’ ) su

Question

At normal atmospheric pressure of 1.00 atm, solid carbon dioxide (‘dry ice’ ) sublimes directly into a gas at -78.5oC. Given the following data and constants, calculate the amount of heat energy, in Joules, needed to heat an 88.0-gram sample of CO2(s) from -100.0oC to its critical point temperature of 31.0°C.

Part 1:

How many Joules of heat are necessary to warm solid CO2 sample from -100.0oC to -78.5oC?

Part 2:

How many Joules of heat are necessary for the solid CO2 sample to sublime to a gas at -78.5oC?

Part 3:

How many Joules of heat are necessary to warm gaseous CO2 sample from -78.5oC to 31.0oC?

Part 4:

What is the total amount of heat energy, in Joules, needed to heat an 88.0-gram sample of CO2(s) from -100.0oC to its critical point temperature of 31.0°C?

For Carbon Dioxide Heat Capacity of Solid, 52.0 J/mol OC Cs(solid) 36.3 J /mol Heat Capacity of Liquid, CI liquid) 25.0 kJ/mol Enthalpy of Sublimation, AHsub

Explanation / Answer

Number of moles of CO2 = mass / molar mass = 88.0 / 44 = 2.00 mol

PART(1):

q1 = ms(t2-t1)

q1 = 2.00 * 52.0 (-78.5 + 100.0)

q1 = 2236 J

PART (2) :

Enthalpy of sublimation , q2= 2.00 * 25.0 * 1000 = 50000 J

PART(3) :

q3 = 2.00 * 36.3 * (31.0 + 78.5)

q3 = 7949.7 J

PART(4)

q = q1 + q2 + q3

q = 2236 + 50000 + 7949.7

q = 60185.7 J

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