🤓 Based on our data, we think this question is relevant for Professor McCamant's class at UR.
The change in internal energy of a system ΔE is related to heat and work by the equation:
Where q is heat and w is work.
The sign of q changes depending on the type of reaction:
(+) q when a system absorbs heat or energy (endothermic)
(-) q when the system releases energy(exothermic)
In the given problem, 40.66 kJ of heat is released when the 1 mole of H2O(g) is condensed to 1 mole of H2O(l). Therefore, the value of q = -40.66 kJ.
Let us now determine the value for work.
One mole of H2O(g) at 1.00 atm and 100.°C occupies a volume of 30.6 L. When 1 mole of H2O(g) is condensed to 1 mole of H2O(l) at 1.00 atm and 100.°C, 40.66 kJ of heat is released. If the density of H2O(l) at this temperature and pressure is 0.996 g/cm3, calculate ΔE for the condensation of 1 mole of water at 1.00 atm and 100.°C.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Internal Energy concept. You can view video lessons to learn Internal Energy. Or if you need more Internal Energy practice, you can also practice Internal Energy practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor McCamant's class at UR.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.