I am having issue with letter b, but the context from letter a is needed to solve. I have provided my answer to a and the steps how I got there. a. Calculate the density of H2O vapor at 1.00 atm and 100.0 °C in g/L. Circle your answer. My work: 100.0 °C + 273 K = 373 K d = (18.01528 g/mol × 1.00 atm)/( 0.08206 L atm mol-1 K-1 × 373 K) d = 18.01528 / 30.60838 d = 0. 589 g/L b. 1.00 mL of water at 25 °C is heated to 100 °C, at which point it boils at an atmospheric pressure of 1 atm and is vaporized. What is the difference in volume (in mL) when this happens? (At 25 °C, liquid water has a density of 0.997 g/mL.) Circle your answer.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
I am having issue with letter b, but the context from letter a is needed to solve. I have provided my answer to a and the steps how I got there.
a. Calculate the density of H2O vapor at 1.00 atm and 100.0 °C in g/L. Circle your answer.
My work:
100.0 °C + 273 K = 373 K
d = (18.01528 g/mol × 1.00 atm)/( 0.08206 L atm mol-1 K-1 × 373 K)
d = 18.01528 / 30.60838
d = 0. 589 g/L
b. 1.00 mL of water at 25 °C is heated to 100 °C, at which point it boils at an atmospheric pressure of 1 atm and is vaporized. What is the difference in volume (in mL) when this happens? (At 25 °C, liquid water has a density of 0.997 g/mL.) Circle your answer.
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