Olive oil lowers “bad” (lower density lipids). Olive oil melts at -6.60 0C and boils at 300.00 0C. The specific heat of liquid olive oil is 2.00 J/g•0C. The specific heat of solid olive oil is 0.850 J/g•0C. If a sample of liquid olive oil at 5.00 0C and warmed to its boiling temperature at 300.00 0C required a total energy of 4.5X103J, what is the heat of vaporization for olive oil? Show the work to logically support your choice. Report the answer to the appropriate significant figures and units of measure.

The specific heat capacity of liquid mercury is 0.14 J g¹ K-¹. How many joules of heat are needed to raise the temperature of 4.00 g of mercury from 19.0°C to 39.5°C? 33 J O 11 J O 0.72 J 0.0017 J 5.9 x 10² J

Consider the following specific heats of metals in the table below. If the same amount of heat is added to 25.0 g of each of the metals, which are all at the same initial temperature, which metal will have the highest temperature? Metal Specific Heat Aluminum 0.897 J/°C'g Magnesium 1.02 J/°C•g Tungsten 0.134 J/°C·g Silver 0.237 J/°C•g Bismuth 0.123 J/°C•g Aluminum Magnesium Tungsten Silver Bismuth

What is the final temperature (in °C) of 500.1 g of water (specific heat = 4.184 J/g.°C) at 24.20°C that absorbed 950.0 J of heat?

1. What is the specific heat of a 10. g sample of a substance that requires 950 J of heat to raise its temp from 18 °C to 42 °C? 2. Hg has a specific heat of 0.14 J/g°C. How much energy does a 22.8 g sample of mercury lose as its temp goes from 33 °C to 16 °C?

A piece of metal weighing 50 grams was heated to 100°C and then dropped into 250 grams of water at 25°C. The metal cooled down and the water became warmer until both were at a temperature of 28.8°C. Calculate the amount of heat absorbed by the water. Assuming that the heat lost by the copper was absorbed by the water, what is the specific heat of the metal? (sH2O = 4.18 J / g °C)

In the above image, you have a solid at less than 0 oC. As you add heat (Q), the temperature of the solid increases until it hits a point when it would start melting. In the case of water, this is at 0 oC. Notice that at this point the temperature stops rising and we have a mixture of solid/liquid. We are still adding heat but the temperature is not changing. Once all of our solid becomes liquid, the temperature starts to rise again until it hits another plateau, at 100 oC. This is the point where the water boils and starts becoming a gas. Again, we add heat but the liquid/gas mixtures temperature does not change. Once all the liquid has become gas, the temperature will start to rise again. Is it possible to have 0 oC water and 0 oC ice?   Yes or No?

How much heat (in kilojoules) is gained by 294 grams of water that is warmed from 25.00C to 57.00C? The specific heat of water is 4.184 J/(g 0C).

Calculate the heat absorbed when 117 g of liquid ethanol at 25.0°C is converted to gaseous ethanol at 96.0°C. The boiling point of ethanol is78.4°C,the specific heat of liquid ethanol is 2.44 J/(g°C), the heat of vaporization of ethanol is3.86×104 J/mol,and the specific heat of gaseous ethanol is 1.42 J/(g°C). enter answer in scientific notation

How much heat is needed to raise the temperature of a 2.5 g piece of copper wire from 20. °C to 80. °C? How much heat is needed to increase the temperature of an equivalent mass of aluminum by the same amount? Once heated, which metal will cool faster?