When 20 calories of heat is added to 2.0 grams of water at 15 degrees Celsius the temperature of water increases to   (Specific heat of Water = 1 calorie/gram °C OR 4.186 joule/gram °C) Select one:     25 degrees Celsius 15 degrees Celsius 5.0 degrees Celsius 50 degrees Celsius

Q: Air 1.01 J/g degrees Celsius Copper 0.385 J/g degrees Celsius NaCl 0.864 J/g degrees Celsius After…

A: Specific Heat Capacity is the amount of heat required to raise the temperature of 1 gram of…

Q: How many calories of heat does it take to change the temperature of 464.4 g of ice from -49.6…

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Q: If 20.0 g of copper cools from 35.0°C to 32.8°C and loses 38.6 Joules of heat, what is the specific…

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Q: If you combine 260.0 mL of water at 25.00 °C and 130.0 mL of water at 95.00 °C, what is the final…

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Q: How many calories of heat (energy) would it take to heat 25.0 g of water from 35.0 °C to 45.0 °C?…

A: Given, Mass of water(m)= 25g Final temperature = 45°C Initial temperature = 35°C Temperature…

Q: A sample of aluminum absorbs 11.2 J of heat and its temperature increased from 23.2°C to 57.5°C.…

A: We know that heat absorbed  by Al  q = m*s*ΔT where q = heat absorbed  by Al; m= mass of Al; s =…

Q: You heat 2 g of water from 25 °C to 26 °C. How many calories of energy are transferred to the water?…

A: Given:  Mass of water = 2g  ∆T = 26-25 = 1°C  Cwater = 1 cal/g°C

Q: 8.2 °C to 34.5 °C? (The

A: Here mass in kg, so first converted mass kg to g  mass = 6.98 kg  [ 1kg = 10^3 g ]  mass = 6.98 •…

Q: The initial temperature of a 22-g sample of copper is 25°C. If the sample absorbs 236 J of heat,…

A: Provided initial temperature of copper(T1) =25°C Let final temperature of copper=T2 Absorbed heat…

Q: The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to…

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Q: Water has a heat of fusion of 80.0 calories per gram .  If I have 8.62 grams of ice at its melting…

A: Answer

Q: What is the specific heat of an unknown liquid if heating a 15.0 g sample with 200.0 J of heat…

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Q: How much heat (in kJ) is needed when 133.43 g of water warms and boils from 33.45°C to 100°C?

A: The mass of the water sample is = 133.43 g The initial temperature of the water is = 33.45oC The…

Q: Calculate the calories needed to heat 7.9 grams of water from 15 degrees Celsius to 33 degrees…

A: Mass of water (m) = 7.9 g Initial temperature (Ti) = 15°C Final temperature (Tf) = 33°C Calories…

Q: How many joules are required to heat 180g of water from 20c to 35c. The specific heat of water is…

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Q: A 75.0 gram sample of a metal is heated until it is at 100.0℃. A calorimeter contains 100.0 grams of…

A: Given that : Mass of sample of the metal (ms)= 75.0 g Its temperature = 100°C Mass of water in the…

Q: How many grams of water at 100 c could be changed from liquid to gas if 4320 calories of heat were…

A: Here we have to use standard value of heat of vaporization of water. Using that value we can…

Q: The specific heat of Uranium is 0.12 Joules / Uranium x Celcius. Convert the specific heat of…

A: Given :  Specific heat of  uranium = 0.12 Joules / gram x Celsius

Q: How many grams of water at 17 °C  must be mixed with 180 g (about 6 oz) of coffee at 96 °C so that…

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Q: Calculate the joules to heat 78g of water from 22°C to 62°C.

A: Mass of water = 78 g Initial temperature , Ti=22°C Final temperature , Tf= 62 °C

Q: Metal Specific Heat (J/goC) Calcium 0.647 Iron 0.449 Silver 0.235 Gold 0.129 Refer to the…

A: Given: The mass of the sample = 55.5 g The amount of heat absorbed = 0.500 kJ The increase in…

Q: If you combine 400.0 mL of water at 25.00 °C and 130.0 mL of water at 95.00 °C, what is the final…

A: This numerical will be solved using the heat equilibrium formula that is given as:…

Q: How many joules of energy is absorbed to drop the temperature of 75 grams of water from 70 degrees…

A: The following formula can be used to calculate the energy absorbed: q = mcΔT=mc[T2-T1] where q:…

Q: What is the final temperature if 21.9 kJ of heat is added to 84.1 grams of water at 24 degrees…

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Q: How many joules of heat are needed to raise the temperature of 10.0g of aluminum from 22 degrees…

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Q: A student places a block of hot metal into a coffee cup calorimeter containing 163.5 g of water. The…

A: Equation for the heat absorbed ( q )   q  =  m  ×  C  ×  ΔT  m = mass C = Specific heat capacity ΔT…

Q: how many calories are required  to raise  the temperature of (2.6x10^2)h of water from 42.0celsius…

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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: If 132 g of ice at 0.0°C is added to 1.64 L of water at 98°C, what is the final temperature of the…

A: a) Given: Mass of ice = 132 g. Initial temperature of ice = 0.0 oC Volume of water = 1.64 L = 1640…

Q: If 300 g of water at an initial temperature of 30°C absorbs 750 J of heat, what is the final…

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Q: Calculate the amount of heat needed to raise the temperature of 55g of liquid water from 25 degrees…

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Q: Calculate the heat capacity of a brick if 100. g sample absorbs 2439 J of heat, and it’s temperature…

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Q: If you combine 310.0 mL of water at 25.00 °C and 140.0 mL of water at 95.00 °C, what is the final…

A: Given :-  First volume = 310.0 mL  First Temperature = 25.00°C  Second volume  = 140.0 mL  Second…

Q: How many joules of heat are released when 10.0 g of aluminum is cooled from 55.6°C to 22.0°C, if the…

A: Q = m . s . (T1 - T2) Where, Q = heat released in J m = Mass of metal in g s = specific heat of…

Q: calculate the heat lose (in Joules) by 115 g of water as it cools from 71.4 C to 34.4 C

A: Given data, Mass of water = 115 g Initial temperature = 71.4oC Final temperature = 34.4oC

Q: calculate the heat required to change the temperature of 15.0 g Fe from 18.5 celsius to 56 .8…

A: Heat required by compound is determined by the knowledge of its mass, its specific heat capacity and…

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…