Determine the specific heat of 122 grams of an unknown substance if it absorbed 270 kJ of heat as it was heated from 25 C to 230 7.12 J/g°C 2.87 J/g°C 10.8 J/g°C 0.01 J/g C

Q: A patient arrives in the emergency room with a burn caused by steam. Calculate the heat that is…

A: given : mass m = 15 g and 2260 Joules per gram. Hence, 2260 × 15 = 33900 J calculate heat released ?…

Q: A compound with a specific heat of 1.26 is at 20.6 degrees C. When 686.8 J of heat are applied to…

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Q: How much heat is absorbed when 1434 grams of ice melts at its melting point. The heat of fusion of…

A: Heat of fusion is defined as the amount of energy required to convert one mole of a solid to liquid.…

Q: How much energy is required to raise the temperature of 10.8 grams of solid chromium from 21.5…

A: According to thermodynamics: q=mc∆T                  . . . (1) Here, m is the mass = 10.8 g c is the…

Q: Water has a heat of fusion  at 80.0 cal per gram. If I have 4.14 g of ice at its melting point how…

A: Heat of fusion is 80 cal/g. We have 4.14 g of ice at 0°C. We have to calculate the heat required to…

Q: How many joules are needed to boil 28.1 g of water if the heat of vaporization is 2256 J/g? . If you…

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Q: An ice bag containing 325g of ice at 0 degrees Celsius was used to treat sore muscles. When the bag…

A: When an ice is melted and convert into liquid, some amount of energy is absorbed.And this…

Q: Assuming that Coca-Cola has the same specific heat as water [4.18 J/(g⋅∘C)J/(g⋅∘C)], calculate the…

A: given, specific heat (c) = 4.18 J/(gm.°C) mass of the substance(m) = 350 gm initial temperature=…

Q: how many grams of water  would require 2.20 x 104 calories of heat to raise its temperature from…

A: Using formula for specific heat we have solved this problem.

Q: Determine the specific heat of a sample of Cu from the fact that 64.0J are needed to raise the…

A: Calculating Specific heat: mass of Cu = m = 15.0 g Specific heat of Cu = = ? J/g°C Temperature…

Q: A metal with a specific heat of 0.780 J/g degrees C requires 45.0 J of heat to raise the temperature…

A: The amount of heat released or absorbed by the substance is calculated by the formula,…

Q: 5) The specific heat of water is: A. 5 Cal per g per C B. 2 Cal per g per C C. 3 Cal per g per C D.…

A: Introduction: The heat capacity of a matter is the quantity of heat required to increase the…

Q: 5. How much heat must be,removed from 15.5 g of water at 90.0°C to cool it to 43.2°C? 30353

A:

Q: Calculate the change in temperature of 10 kg of water released 232 kJ of heat

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Q: Why does liquid water have a higher specific heat than ice or water vapor?     a Liquid water is…

A: Heat capacity is the capacity or the measure to sustain heat via a fixed amount of substance. Since…

Q: The specific heat of ice is 0.492 cal /(g x °C). How many calories of heat are required to raise the…

A: Given: Specific heat capacity of ice= 0.492 cal/g⋅ oC Mass of ice = 100.0 g Initial Temperature of…

Q: How much heat is involved when an 100 g ice at 0 °C is heated to 80 °C? Specific heat of ice is 0.5…

A: Given: Mass of ice is 100 g. Specific heat of ice is 0.5 cal/g·°C. Temperature is heated from 0°C to…

Q: How much heat is needed to melt 23.8 g of copper that is at an initial temperature of 21.7 °C? The…

A: The heat of a solution can be expressed by the following formula   Q=mCΔT Q=heat m=mass C=heat…

Q: An eager scientist on a hot summer day needs to determine how much ice to buy. She has a cooler…

A: The Initial temperature of soda = 86.5 ◦F The Final temperature of soda = 40.8 ◦F Conversion of…

Q: The specific heat capacity of liquid mercury is 0.14 J/gK. Calculate the amount of heat in are…

A: Specific heat capacity is the amount of heat that needs to increase the temperature by 1 oC of a 1 g…

Q: Calculate the number of calories released when 32.0 g of water cools from 95.0 C to 20.0 C. The…

A: Since the heat of the process is given by  Q = mCΔT  where Q = heat involved  m = mass = 32 g C =…

Q: Calculate the amount of heat needed to boil 30.2g of water (H2O), beginning from a temperature of…

A: Specific heat capacity is the heat that must be applied to increase the temperature of 1 g of the…

Q: How much heat is required to warm 1.50 kg of sand from 24.0 ∘C to 100.0 ∘C

A: Given: Mass of water = 1.5 kg = 1500 g Initial temperature (T1) = 24°C  Final temperature (T2) =…

Q: If 9000.0J of heat are absorbed by 800.0 g of water at 5.0 degree C, what will be its final…

A: Given,  If 9000.0J of heat are absorbed by 800.0 g of water at 5.0  °C, the final temperature of…

Q: the specific heat of diethyl ether is 2.33 j/g celsius if 113j of heat raises the temperature of a…

A: Specific heat of diethyl ether = 2.33J/g°C Q = amount of heat released = 113J Mass = 12.5g Tf =…

Q: The heat of fusion for water is 80 calories / Gram in the heat of vaporization for water is 540…

A: Heat of fusion is the amount of energy which is required to convert ice into the water at the same…

Q: How much heat is gained when you raise the temperature of an ice cube that weighs 4.46 grams from…

A: Hence the energy required in each process is given by  1) heating of ice from –4.0 °C to melting…

Q: The temperature of an object increases by 24.4 °C when it absorbs 3725 J of heat. Calculate the C =…

A: The specific heat capacity for a given chemical substance or a solution refers to the amount of the…

Q: How much heat is liberated when 50g of water is cooled from 100 ᵒ C to 20 ᵒ C

A: This can be solved as follows

Q: 5. A 85.75g sample of a clear liquid is cooled from 68.3° to 32.1°C when it loses 5850 Joules of…

A: Specific heat capacity is amount of heat needed to increase the temperature of one gram of substance…

Q: The temperature of a sample of water increases from 20.0°C to 46.6°C as it absorbs 5650 J of heat.…

A: Given,  Initial temperature = Ti = 20.0 °C Final temperature = Tf = 46.6 °C Amount of heat absorbed…

Q: A burning chip causes 85 g of water to rise from 5.5 C to 16.5 C. The specific heat of water is 1.00…

A: Mass(m) = 85g C= 1cal/gc T = T2 - T1 =  16.5 - 5.5 = 11Celsius Formula used q = mc(T2 - T1)

Q: How much heat, in kJ, is absorbed by 50.0g of water if the temperature changes from 298K to 357K?…

A: Given, The amount of heat absorbed by 50.0g of water to increase temperature from 298 K to 357 K is:

Q: How much heat is gained by Aluminum when 52.2 g of Al is warmed from 20.3D defrees Celsius to 35.1…

A: Given, mass of Al (m) =52.2 gInitial temperature T1 =20.3°CFinal temperature T2 = 35.1°Cspecific…

Q: How much heat would need to be removed to cool 192.7 g of water from 25.6°C to -10.7°C? Csolid =…

A: Heat released = 24.954 kJ

Q: 6. If the same amount of heat is added to 25.0 g sample of each of the metals in the chart below,…

A: Given,  If the same amount of heat added to 25.0 g sample of each of the metals, the metal which…

Q: heat. The initial temperature of water is 56.23 degrees celsius. Calculate the final

A: Heat (q) = ms.□T Where,  q = Heat = -523.9 J (negative sign is used as heat released)  m = mass of…

Q: how many joules of heat are required to heat 25.0 g of ethyl alcohol from The prevailing room…

A: Consider the given information is as follows; Mass of ethyl alcohol (m) = 25.0 g    Initial…

Q: heat

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Q: Calculate the quantity of heat absorbed by 30.0 g of water when its temperature is raised to 67.9…

A:

Q: How much heat is required to warm 2.07 kg of sand from 32.6 to 48.9 °C. The specific heat of sand is…

A:

Q: Calculate the amount of heat released when a 225g sample of gold cools from 86.0C to 32.5C. The…

A: The amount of heat released from given grams of gold is determined by using Q = mc deltaT.

Q: How much heat is gained by nickel when 213 g of nickel is warmed from 22.2 °C to 59.0 °C. J The…

A: Interpretation: Heat gained by nickel when 213 g of nickel is warmed from 22.2 oC to 59.0 oC is to…

Q: A 50.0 g sample of water at 70.0 °C is mixed with 60.0 g of water at 20.0 °C. Find the final…

A: System is isolated that means No heat is transferred from the system on sorrounding On Mixing of…

Q: How much heat would be required to raise 499 g of water from 111 °C to 251 °C? (You need to know…

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Q: In which state (×) does a gram of water loses more heat to cool down to +20 °C?   ___ (l) at +100…

A: 1) Given: Final temperature of water = 20 oC.

Q: Calculate the amount of heat needed to raise the temperature of 55.0 g of liquid water from 25°C to…

A: The mass of liquid water is = 55.0 g The initial temperature of the liquid water is = 25°C The final…

Q: A 30.37 g sample of a substance is initially at 28.3 degrees Celsius. After absorbing 2235 J of…

A: The amount of heat (Q) gained or lost by a substance (with mass m) as its temperature changes (ΔT)…

Q: What is the mass of a sample of liquid water that took 35.4 kJ of heat to apply to it to raise its…

A: Answer: option b. 257 g if the mass of a sample of liquid water.

Q: amount of heat released

A:

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates). 

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.