6. What does the temperature change as liquid water is warming up? a. What type of energy is changing during this process? How do you know? Is it increasing or decreasing? b. What type of energy is staying constant during this process?

QUESTION 39 In measuring the specific heat of water, which of the following statements is true?    a. The measurement is always done at room temperature.    b. Heat sources are difficult to calibrate, and therefore high-quality measurements are difficult.   c. Isolating the experiment from the outside environment is important to obtain reasonable results.    d. Since energy is conserved, the measurements don’t depend on how long you wait before you measure the temperatu

1. Water has a specific heat of 4.184 J/g°C while glass (Pyrex) has a specific heat of 0.780 J/g °C. If 10.0 J of heat is added to 1.00 g of each of these, which will experience the larger increase of temperature? a. Glass b. Water a b d c. They both will experience the same change in temperature since only the amount of a substance relates to the increase in temperature. d. There is not enough information provided to answer this question

A reaction is endothermic if it  A. absorbs heat  B. does work  C. has work done on it  D. releases heat

an a. Aluminum (specific heat capacity of 0.921 J/g°C) b. Copper (specific heat capacity of 0.377 J/g°C) c. Stainless Steel (specific heat capacity of 0.502 J/g°C) From the metals, what is your best guess for the of the metal? temperature of the at as the specific heat of water.

0. A 1.325 kg sample of Compound Y absorbed 5.65 kJ of heat. If the final temperature is 52.3°C, what was the initial temperature? Use your average specific heat for Compound Y.

When the same amount of heat is applied to both, which will heat up to a higher temperature—a given mass of water or that same total mass of water and steel together? Why?

Equal masses of copper, aluminum, iron, silver, and water absorb equal amounts of heat. Which substance will undergo the smallest increase in temperature?   a. Iron   b. Copper   c. Silver   d. Aluminum   e. Water

The specific heat of aluminum is 0.214 cal/g.°C. Determine the energy, in calories, necessary to raise the temperature of a 55.5 g piece of aluminum from 23.0 to 48.6°C. A. 109 cal B. 273 cal C. 577 cal D. 347 cal E. 304 cal Energy is the ability to do work and can be: A. converted to one form to another B. can be created and destroyed C. used within a system without consequences D. none of the above

5. Why does the temperature stay constant as the ice melts into water and as the water boils to a gas (during the phase changes)? a. What type of energy is changing during these processes? Is it increasing or decreasing? b. What type of energy is staying constant during these processes? How do you know?