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The specific heat of water is 4186 J/kg·°C due to its molecular structure and hydrogen bonding, which requires a significant amount of energy to increase the temperature of water. This high specific heat allows water to absorb and store large amounts of heat without a substantial increase in temperature, making it an effective temperature regulator in natural and biological systems. Additionally, this property plays a crucial role in climate regulation and homeostasis in living organisms.
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How does the phrase of water affect its specific heat capacity?
It is because the density increases as you add salt and with all other substances the higher the density the lower the specific heat. For example water has a density of 1000 Kg m -3 and a specific heat of 4186 J/Kg. On the other hand copper has a density of 8960 Kg m -3 and a specific heat of 385 J/Kg.
Why specific capacity of water equals 4186J?
The specific heat capacity of water is 4186 J/kg°C because water requires a large amount of energy to change its temperature due to the hydrogen bonds between water molecules. This property makes water an effective temperature buffer in nature, regulating the Earth's climate and supporting life.
What is the heat required to raised the temperature of 0.6 kg of water from 30 degrees to 40 degrees?
Using the formula H=mS(t2-t1) we get H=0.6 x 1x 10=6 KJ of heat. Here H is heat, m is mass of substance, S is specific heat capacity of substance, t2 final temperature and t1 is initial temp.
Why would hydrogen make a better coolant than water?
Water is called a universal coolant because it can cool the machines which has been so hot after the process.the water is pumped into the machine where it comes out as steam which can be used for other purposes.The steam has a lot of energy taken from the machines. So nice ah............
What mass of water is required to absorb 4.7 times 10 5 J of energy from a tea kettle while the temp increases from 302K to 357K the specific heat of water is 4186J kg?
0.20 Kg or 200 g Specific heat is 4186 J * Kg * Change in temperature of either K or C Thus Kg = 47000 J / (4186 J * 55 K) = .20 Kg The answer to four digits is 0.2041, but the amount of joules you have only has two significant figures, so the final answer would only have two significant figures.
What is the specific heat of water in joules per kilogram degree Celsius?
The specific heat of water is 4186 joules per kilogram degree Celsius.
Specific heat of blood?
4186 J/(kg C)
How much heat is contained in 100 kg of water at 60.0 C?
The amount of heat contained in 100 kg of water at 60.0°C can be calculated using the formula Q = mcΔT, where Q is the heat energy, m is the mass of water, c is the specific heat capacity of water, and ΔT is the change in temperature. Given that the specific heat capacity of water is 4186 J/kg°C, the heat contained in 100 kg of water at 60.0°C would be Q = 100 kg × 4186 J/kg°C × (60.0°C - 20.0°C).
What is the amount of heat needed to raise that temperature of 1 kilogram of water 1 degree Celsius?
The amount of heat needed to raise the temperature of 1 kilogram of water by 1 degree Celsius is 4186 Joules, which is the specific heat capacity of water.
How much heat in joules would you need to raise the temperature of 1kg of water by 5 and degC?
You would need 20,920 Joules of heat to raise the temperature of 1kg of water by 5°C. This value is calculated using the specific heat capacity of water, which is 4186 J/kg°C.
How much heat is required to raise the temperature of 0.25 kg of water from 20 Celsius to 30 Celsius?
The specific heat capacity of water is 4186 J/kg*C. To calculate the heat required, use the formula: heat = mass * specific heat capacity * change in temperature. Plugging in the values, the heat required to raise the temperature of 0.25 kg of water by 10 degrees Celsius is approximately 1046.5 Joules.
What is the amount of heat needed to raise the temperature of 1kilogram of water 1degrees Celsius?
The specific heat capacity of water is 4.18 J/g°C. Therefore, it would require 4186 Joules (4.18 x 1000 grams) of energy to raise the temperature of 1 kilogram of water by 1 degree Celsius.
How much heat is needed to raise 8 kg of water from 4 degrees Celsius to 83 degrees Celsius?
The heat needed can be calculated using the formula: Q = mc∆T, where Q is the heat, m is the mass of water, c is the specific heat capacity of water (4186 J/kg°C), and ∆T is the change in temperature. Plug in the values to find the heat needed.
How does the phrase of water affect its specific heat capacity?
It is because the density increases as you add salt and with all other substances the higher the density the lower the specific heat. For example water has a density of 1000 Kg m -3 and a specific heat of 4186 J/Kg. On the other hand copper has a density of 8960 Kg m -3 and a specific heat of 385 J/Kg.
What is the specific heat value of ice?
* Specific heat capacity water liquid 4186 J/kgK "typical" ... 4210 J/kgK @ 275 K ; minimim 4178 J/kgK @ 308 K ; 4215 @ 370 K * Specific heat capacity water solid is 2050 J/kgK@ 270 K, drop to 1392 J/kgK @ 175 K * Specific heat capacity water vapor is 1890 J/kgK @ 375 K, up to 2000 J/kgK @ 575 K
Why specific capacity of water equals 4186J?
The specific heat capacity of water is 4186 J/kg°C because water requires a large amount of energy to change its temperature due to the hydrogen bonds between water molecules. This property makes water an effective temperature buffer in nature, regulating the Earth's climate and supporting life.
What is the heat required to raised the temperature of 0.6 kg of water from 30 degrees to 40 degrees?
Using the formula H=mS(t2-t1) we get H=0.6 x 1x 10=6 KJ of heat. Here H is heat, m is mass of substance, S is specific heat capacity of substance, t2 final temperature and t1 is initial temp.
