Thermochemistry: Heat Absorbed; Specific Heat Capacity & Change In States

If 80 grams of water is heated from 26^oC to 31^oC, how much heat is absorbed? (C_p of liquid water = 4.184 J/g^oC) (Heat absorbed/lost q) m = (mass m ) (change in temperature ∆ t) (specific heat capacity C_p)

A piece of aluminum (3.6 g) is heated from 20^oC to 30^oC. If the specific heat of aluminum os 0.897 J/g^oC, how much heat energy was absorbed?

A 34 gram piece of an unknown metal absorbs 351.56 Joules of energy when the temperature increased from 10^oC to 32^oC. What is the specific heat of the substance? Hint: You are solving for Specific Heat (C_p) not heat absorbed.

A 33.3 gram piece of iron (Cp 0.449 J/gC) absorbs 290.0 J of energy. What was the increase (change in temperature) in degrees celsius?

A 6.8 g sample of glass was heated from 4 C to 39 C. It was found to have absorbed 59.5 J of energy. What is the specific heat of this type of glass?

A 42.6 gram pie ce of metal is heated to a temperature of 100 C. A 250 ml container of water (recall 1 g of water = 1 ml) starts at a temperature of 17 C. When the metal is added to the water, the water increases in temperature to 20 C. (The  specific heat capacity of water is 4.184 J/g C) What is the specific heat capacity of the metal? Assume a closed system. How to aproach the problem: Write what you know about the water and about the metal: Water: Change in temperature 17 to 20; 250 g; 4.184 J/gC Metal: Change in temperature 100 to 20; 42.6g ; Cp unknown Recall that the heat lost by the metal will equal the heat gained by the water in a closed system. Since the change in temperature, mass and specific heat capacity of water are all known, solve for heat abosrbed by water first: Heat absorbed by water= (3 C) (250) (4.184). This answer will be the SAME as the heat lost by the metal. 3,138 J of heat lost by water (or gained by metal). Now go to metal side. Use the 3,138 J from the water equation for the heat lost from the metal. 3,138 J = (100-20 C) (42.6 g) (Cp) . Now solve for the Cp of metal

A 96.85 g piece of metal is heated to a temperature of 100 C. A 250 ml container of water( recall: 1 g of water = 1 ml of water) metal is added to the water, the water increases in temperature from 13 C to 19 C. (The specific heat capacity of water is 4.184 J/g C). What is the specific heat capacity of the metal? Assume a closed system. How to approach this problem: Write what you know about water and about the metal. Remember that the heat lost from the metal is gained by the water. Solve frist for the heat absorbed/loss on the side without unknowns (i.e. water).

Whichtemperature represents the heat of vaporization? (Hint: Change in state: (Ex: Solid to liquid; liquid to gas) will NOT have an increase in temperature.

Which area on this graph represents a substance that is completely a gas?

If 100 grams of water is heated from 19 C to 23 C how much heat is absorbed? Cp water = 4.184 J/gC