Author Question: The enthalpy change for converting 1.00 mol of ice at -60.0C to water at 80.0C is The specific heats ... (Read 73 times)

shofmannx20 · **on:** Nov 18, 2019

Question 1

Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) at 35.0 °C to gaseous CCl4 at 76.8 °C (the normal boiling point for CCl4). The specific heat of CCl4(l) is

its heat of fusion is

and its heat of vaporization is

◦ 6.28 kJ
◦ 1.43 kJ
◦ 0.896 kJ
◦ 5.74 kJ

Question 2

The enthalpy change for converting 1.00 mol of ice at -60.0°C to water at 80.0°C is

The specific heats of ice, water, and steam are

and

respectively. For H₂O,

= 6.01 kJ mol-1, and

.
◦ 14.29
◦ 13.17
◦ 48.95
◦ 9.77
◦ 8282

Pamela.irrgang@yahoo.com · **Reply #1 on:** Nov 18, 2019

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