QUESTION 10 What mass of water can be heated from 25.0° C to 50.0° C by the addition of 2.825 kJ? (specific heat of water = 4.184 J/°C *g) q = mcAT ○ 2.70 x 10-2 g 27.0 g ○ 1.40 x 10-2 g 14.0 g

How many Joules of energy are required to raise 2.5kg of water from 18.5 to 55.0 ? (specific heat of water is 4.184J/g C) in correct sig fig

(multiple choice question, choose one) A piece of Titanium weighing 252 grams, and at a temperature of 76 oC, is placed in a calorimeter containing 175.0 grams of water at 21.9oC, the temperature of the water is increases to what if the specific heat of the calorimeter is 29.5J/K? a.) 29.201 C b.) 30.5 C c.) 28.52 C Specific heat titanium 0.523 Specific heat water 4.184

Examine the experimental data below: 1st type of unknown metal Mass of cup and water:                            170.54 g Mass of cup:                                             6.83 g Initial temperature of water:                    24.0OC Final temperature of water:                     26. 0OC Mass of unknown metal:                          21.95g Initial temperature of unknown metal:    100.0OC Final temperature of unknown metal:      26.0OC   Questions: 1. Calculate the heat gained by the water in the calorimeter. Note that the temperature of the cup did not change. 2. Calculate the specific heat of the unknown metal, using the heat gained=-heat lost equation. 3. Look up for the list of specific heat values of some metals in the internet. Compare your experimental specific heat value to other metals’ specific heat. What do you think is the name of the unknown metal?

41. A 25.0 g mercury is heated from 25 °C to 155 °C and absorbs 455 J of heat in the process. What is the specific heat of mercury? Group of answer choices 0.250 J/g °C 0.130 J/g °C 0.140 J/g °C 0.444 J/g °C

How much heat, in joules, is required to raise the temperature of 35.6 grams of iron from 101.0 °C to 170.0 °C ? The specific heat of iron is 0.444 J/g°C.    Question 19 options:   1080.6 J   1090.6 J   1906.0 J   1096.0 J   1190.6 J

Question 1: We have a bomb calorimeter with a heat capacity of 555 J/K. In this bomb, we place 1000.0 mL of water. 2.110 g of a solid are burned in the bomb calorimeter. The temperature 2.17 deg*C of the bomb and water increases by The molar mass of this solid is 538g/m*ol How much heat would be released (in kJ, and note that we want the amount of heat released ) if we burned 0.125 mol of this solid in the bomb calorimeter? The specific heat of water is 4.184J/K/g Make the approximation that the density of water is 1g/m*L

What is the ∆ T for 40.0 grams of water that absorbs 1400 scientific calories at room temperature?   Given:  Heat = (grams)(specific heat)(∆ T)  where specific heat = 1.00 calorie/g°C

1. The specific heat of copper is (0.0924 cal/go C), how much energy is required to raise the temperature of 10.0 g of copper by 100.0 o C? Answer: 92.4 cal 2. If 25.6 J of energy raised 786 g of a substance from 20.0o C to 35.0o C, what is the specific heat of the substance (S)? Answer: 2.17 x 10-3 J/g o C

QUESTION 2 What is the specific heat capacity of Al if 991.5 J were required to heat 35.83 g of it from 25.0°C to 55.68 °C? Key Concept:: Calorimetry. When a substance is heated, the heat absorbed is equal to the product of mass of substance being heated times the temperature change times the specific heat capacity, q = s*m*ΔT