fy the phase changes as endothermic or exothermic. Endothermic solid to liquid liquid to gas solid to gas liquid to solid Answer Bank show work. don't give Ai generated solution Exothermic gas to liquid gas to solid

The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.

How many grams of water at 0C will be melted by the condensation of 1 g of steam at 100C?

A calorimeter contains 72.0g of water at 19.2C. A 141-g piece of tin is heated to 89.0C and dropped into the water. The entire system eventually reaches 25.5C. Assuming all of the energy gained by the water comes from the cooling of the tin-no energy loss to the calorimeter or the surroundings-calculate the specific heat of the tin.

Sublimation is the phase change from solid to gas without going through a liquid phase. Solid CO2, called dry ice, is an example of one substance that sublimed. Use Hesss law to show that the enthalpy of sublimation, subH, is equal to fusH vapH.

Open the PhET States of Matter Simulation (http://openstaxcollege.org/l/16phetvisual) to answer the following questions: (a) Select the Solid, Liquid, Gas tab. Explore by selecting different substances, heating and cooling the systems, and changing the state. What similarities do you notice between the four substances for each phase (solid, liquid, gas)? What differences do you notice? (b) For each substance, select each of the states and record the given temperatures. How do the given temperatures for each state correlate with the strengths of their intermolecular attractions? Explain. (c) Select the Interaction Potential tab, and use the default neon atoms. Move the Ne atom on the right and observe how the potential energy changes. Select the Total Force button, and move the Ne atom as before. When is the total force on each atom attractive and large enough to matter’? Then select the Component Forces button, and move the Ne atom. When do the attractive (van der Waals) and repulsive (electron overlap) forces balance? How does this relate to the potential energy versus the distance between atoms graph? Explain.

A quantity of ice at 0C is added to 64.3 g of water in a glass at 55C. After the ice melted, the temperature of the water in the glass was 15C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C).

On a hot day, you take a six-pack ot a on a pcmc, cooling it with ice. Each empty (aluminum) can weighs 12.5 g. A can contains 12.0 oz of soda. The specific heat of aluminum is 0.902 J/g C; take that of soda to be 4.10 J/g C. (a) How much heat must be absorbed from the six-pack to lower the temperature from 25.00 to 5.00C? (b) How much ice must be melted to absorb this amount of heat? (Hfus of ice is given in Table 8.2.)

Define the joule in terms of SI base units.

Assume you have 1 cup of ice (237 g) at 0.0 C. Calculate how much heating is required to melt the ice, warm the resulting water to 100.0 C, and then boil the water to vapor at 100.0 C. (Hint: Do three separate calculations and then add the results.)