9. Substance Mass (g) Initial Temperature(°C) AT (°C) Specific Heat Capacity (J/gx°C) Aluminum 20.0 90. -5.9 0.90 ? Water 40.0 25 6 4.2 ? For an experiment, a 20.0 g piece of Al was placed inside an insulated cup filled with 40.0 g of H20. The data are given in the table above. Assuming no heat is absorbed by the container or the surroundings, which of the following equations provides the correct mathematical relationship for the transfer of heat q between Al and H20?

4. Aluminum metal melts at 658.5°C. What would be the final temperature if 28.0 grams of solid aluminum at this temperature were placed into 520 grams of liquid aluminum at 1000.0°C? The heat of fusion for aluminum is 396 J/ -1 -1 g, and the specific heat of liquid aluminum is 0.481 J-g`¹deg-¹. (Note: this is the aluminum analog to the process you just did in lab!)

A 35.0 g sample of bronze (specific heat: 0.402) is left in a deep freezer for several hours then placed into 75.5 g of water (specific heat: 4.184) initially at 25.0 ˚C. The water and the bronze stabilize when both are at 15.5 ˚C. What was the initial temperature of the bronze?

Please fill in the four blanks. Thank you!

ature of a 12.58 g sample of calcium carbonate [CaCO,(s)] decreases from 382 C to 23.6 C the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are lost to the surroundings? Select one: O a. 151 O b. 7.5 OC.-5.0 O d. -0.82 e. -138

When a 45.0 g sample of an alloy at 100.0 °C is dropped into 100.0 g of water at 25.0 °C, the final temperature is 37.0 °C. What is the specific heat of the alloy? The specific heat of H20(1) is 4.184 J'g-1.°c-1. q = mc AT O A. 0.423 J-g-1.°c-1 O B. 9.88 J-g-1.°C-1 O C. 48.8 J'g-1.°C-1 O D. 1.77 Jg-1.°c-1

A sample of 175°C copper is placed into a beaker with 100 grams of 25°C water. Which sample of copper will heat the water to the lowest final temperature? The specific heat of copper is 0.385 J-g-1.°C-1. The specific heat of water is 4.184 J·g-1.°C-1. A. 5.0 g Cu B. 2.0 g Cu C. 0.5 g Cu D. 1.0 g Cu

2. A 20.0 g sample of copper is heated from 20 °C to 1083 °C and half of it is melted at that temperature. The specific heat (sometimes referred to as the specific heat capacity) of copper is 0.385 J g¹K and the heat of fusion of copper is 205 Jg K. How much heat, in kJ, is absorbed by the sample of copper? A) 12.9 B) 8.91 C) 10.2 D) 5.18 E) 6.34

A 52.76 g sample of a substance is initially at 28.4 °C. After absorbing 1985 J of heat, the temperature of the substance is 133.4 °C. What is the specific heat (c) of the substance? c =

A 39.60 g sample of a substance is initially at 23.9 °C. After absorbing 1521 J of heat, the temperature of the substance is 116.6 °C. What is the specific heat (?c) of the substance?