chem test 6/6

A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron.

0.46 J/gx C

How many Joules of energy are required to change 10 gram of ice at -2 C to water at 20 C?

10,140 J

The specific heat of aluminum is 0.21 J/g°C. How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?

105 J

The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?

12.82 C

How much liquid water can you change 20 C if you apply 20,000 J?

250 g

How many Joules of energy are required to change 10 gram of water from 20 C to 90 C?

2800 J

How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/gx°C?

297 Joules

20 g of water. specific heat of water is 4.18 J/x°C. temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings?

418 J

symbol for specific heat

C

Do the reactants in an exothermic reaction have a higher or lower energy than the products?

higher

Do reactants in an endothermic reaction have a higher or lower energy than the products?

lower

high specific heat

requires more energy to change temperature

Amount of energy needed to increase the temperature of 1 gram of a substance by 1*C

specific heat

C

symbol for specific heat

kinetic energy

temperature

unit of thermal energy

J

thermal energy symbol

Q

Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same thermal energy. What material would be the coolest after being heated?

carbon steel

During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel

cold