5.85 g
We have to use Q = m s @
Q - heat energy in joule ie 65.5 J
s - specific heat capacity ie 0.140 J/g/C
@ = @2 - @1 = 100 - 20 = 80 C
Just plug and you get the above 5.85 g nearly
Add:
Q = m•C•Δt, where Q is heat added, m is mass in grams, C is specific heat, and Δt is change in temperature.
Known:
Q = 65.5 Joules
C = 0.140 J/g•oC
Δt = 100oC-20oC = 80oC
Unknown: mass of mercury in grams
Solution
m = Q/C•Δt
m = 65.5 J/(0.140 J/g•oC)(80oC) = 6 grams (rounded to 1 significant figure)
The specific heat capacity is given as 0.140 J/g°C, which means it takes 0.140 J of energy to raise the temperature of 1 g of Mercury by 1°C. To determine the mass of mercury requiring 65.5 J to increase from 20°C to 100°C, you divide the energy by the specific heat capacity: 65.5 J / 0.140 J/g°C = 467.8 g. Therefore, 467.8 g of mercury is needed.
The substance that requires the largest amount of energy to increase the temperature is the one with the highest specific heat capacity. Water has one of the highest specific heat capacities of commonly found substances, so it would require the largest amount of energy to increase the temperature of 20 grams by 1.0 K.
If a substance has a specific heat less than one, it would take less heat to raise its temperature compared to a substance with a specific heat of one. This is because substances with lower specific heat values require less energy to raise their temperature by a certain amount.
Not necessarily. A substance with a high specific heat capacity can absorb a lot of heat energy without a large increase in temperature. This means it can reach a high temperature if it receives enough heat, but its ability to retain heat may delay the rate at which it heats up.
The temperature drop varies among liquids due to differences in their specific heat capacities. Liquids with higher specific heat capacities require more energy to change their temperature, resulting in a smaller temperature drop when heat is removed. Conversely, liquids with lower specific heat capacities exhibit larger temperature drops when heat is extracted.
The term used to describe the amount of energy required to raise the temperature of a substance by one degree Celsius is specific heat.
Not necessarily. A substance with a high specific heat capacity can absorb a lot of heat energy without a large increase in temperature. This means it can reach a high temperature if it receives enough heat, but its ability to retain heat may delay the rate at which it heats up.
Cellurized Mercury
Yes.
Iron would require a greater amount of heat to raise its temperature compared to water. This is because iron has a higher specific heat capacity, meaning it takes more heat energy to increase its temperature by 1 degree Celsius compared to water.
All liquids can be turned into a gas with the correct amount of energy. Assuming the question is specific to liquids at room temperature then the answer is Mercury (Hg) and Bromine (Br).
Yes, materials with a high specific heat can absorb a significant amount of energy when heated because they require more energy to raise their temperature compared to materials with lower specific heat. This property makes them useful for applications like heat storage and temperature regulation.
Higher temperature means greater energy content compared to a lower temperature. The energy required to change the temperature is proportional to the mass of the system, the specific heat capacity, and the temperature change.
A lounge chair would require the least energy to increase its temperature because it has a lower specific heat capacity compared to sand or water. Specific heat is the amount of energy needed to raise the temperature of a substance by 1 degree Celsius. Since lounge chairs are typically made of materials like wood or fabric with lower specific heat capacities, they heat up faster with less energy input compared to sand or water, which have higher specific heat capacities.
Its temperature and its specific thermal capacity
Whichever of them has the lowest specific heat capacity will take the least energy to raise its temperature, and whichever has the highest specific heat capacity will take the most energy.
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