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12 Nov 2019

A 10.3 gram sample of cobalt is heated to 99.85 degrees Celsius in a boiling water bath. The hot metal is then immersed in 20.47 grams of water that is initially at 23.74 degrees Celsius. At what temperature will the water reach thermal equilibrium?

The specific heat of cobalt is 0.421 J/gC and the specific heat of water is 4.184 J/gC

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Nestor RutherfordLv2

12 Sep 2019

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In order to determine the specific heat of an alcohol, 200.00 grams at 12.17 degrees Celsius is combined with 130.00 grams of water at 53.78 degrees Celsius. Once thermal equilibrium is reached, the temperature of the mixture(water and alcohol) is 33.21 degrees Celsius. What is the specific heat of the alcohol?

Specific heat of water is 4.184 J/g *C

A 12-inch diameter ball of pure cobalt metal at 225 degrees Celsius was placed in 10.0 gallon of water at 15 degrees Celsius what is the final temp of the water? (specific heat for Cobalt = .421 J/g degrees Celsius, density of cobalt = 8.862 g/cm^3, 1 gal= 3.785 L, 1in=2.54 cm, V(shpere)=4/3*pi*r^3

1. A 500 gram sample of hot mythril ore is submerged in a cold water bath. If the water experienced a change in heat of -58 kJ and the mythril ore experienced a temperature change of 4 kelvin, what must the specific heat capacity of the ore be? Have answer in units of J/g x degrees Celsius & show steps.

a. -0.43 J/g x degrees Celsius

b. -29 J/g x degrees Celsius

c. 0.029 J/g x degrees Celsius

d. 29 J/g x degrees Celsius

2. The following hypothetical circumstance takes place in a coffee-cup calorimeter. Dissolving 3 moles of a salt in 100 grams of water causes the temperature of the water to increase by 3 degrees Celsius. What is the enthalpy of this reaction? The specific heat capacity of water is 4.184 J/g x degrees Celsius

a. 1.255 kJ/mol

b. -225.9 kJ/mol

c. -0.4184 kJ/mol

d. -0.2259 kJ/mol

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