A student measures the initial temperature of an object as 28.33oC and the final temperature as 62.35 oC. What is the change in temperature in units of Kelvin?

An unknown metal is found to have a specific heat capactiy of 0.235. From this, calculate its molar mass.

What is the relationship between the change in temperature of the objects?

Into a well insulated cup (meaning no heat lost or gained to the surroundings) a sample of water at room temperature is added. To the water, a sample of metal at 80 oC is added.
What object(s) gain(s) energy?

What is the relationship between the final temperatures of the metal and the water?

To find the change in temperature in units of Kelvin, we need to use the Kelvin scale which is based on the Celsius scale. The Kelvin scale starts at absolute zero, which is -273.15 degrees Celsius.

To get the temperature in Kelvin, we need to add 273.15 to the temperature in Celsius.

For the initial temperature:
28.33 + 273.15 = 301.48 K

For the final temperature:
62.35 + 273.15 = 335.5 K

To find the change in temperature, we subtract the initial temperature from the final temperature:
335.5 K - 301.48 K = 34.02 K

So, the change in temperature is 34.02 Kelvin.

To calculate the molar mass of the unknown metal using specific heat capacity, we need to use the formula:

molar mass = specific heat capacity / molar heat capacity

The molar heat capacity represents the amount of energy required to raise the temperature of one mole of a substance by one Kelvin.

Unfortunately, specific heat capacity alone is not enough to calculate the molar mass. We need additional information, such as the molar heat capacity or the mass of the substance.

The relationship between the change in temperature of the objects is that it represents the difference in temperature between the initial and final states. It shows how much the temperature has changed during a process, either increasing or decreasing.

In the given scenario, the water and the metal are both objects being discussed. When the metal at 80°C is added to the water, the water gains energy from the metal, while the metal loses energy to the water. Energy transfer occurs from a higher temperature object (metal) to a lower temperature object (water) as heat flows from a hotter body to a cooler one.

The final temperatures of the metal and the water will approach an equilibrium temperature. This means that eventually, the metal and the water will reach the same temperature, resulting in the heat energy being evenly distributed between them. The final temperature will depend on factors such as the initial temperatures, masses, and specific heat capacities of the metal and the water.

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