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