The same heat transfer into identical masses of different substances produces different temperature changes. Calculate the final temperature when 1.00 kcal of heat transfers into 1.00 kg of the following, originally at 20.0°C : (a) water
Q: A 1.50-kg iron horseshoe initially at 590°C is dropped into a bucket containing 12.0 kg of water at…
A:
Q: A hot lump of 37.4 g of aluminum at an initial temperature of 65.9 °C is placed in 50.0 mL H,O…
A: mass of aluminum piece = 37.4 g Initial temperature of aluminum piece = 65.9oC volume of water = 50…
Q: The same amount of heat entering identical masses of different substances produces different…
A:
Q: What is the heat capacity of a system consisting of 8.10 kg of water in a 0.310-kg aluminum bucket?…
A: Write the given values with the suitable variables. mw=8.10 kgma=0.310 kgCa=0.9 kJ/kg KCw=4.186…
Q: Suppose a person is covered head to foot by wool clothing with average thickness of 2.40 cm and is…
A: CONCEPT:
Q: In an insulated container, you combine hot metal with ice. The ice starts at -20 degrees C. The…
A: Obtain the specific heat of ice. Obtain the specific heat of the water. Obtain the latent heat of…
Q: A 3.00-g copper coin at 25.0°C drops 77.0 m to the ground. (a) Assuming 61.2% of the change in…
A: Given: The mass of the coin is 3.00 g. The initial temperature of the coin is 25 °C. The height of…
Q: (a)How much heat transfer (in kcal) is required to raise the temperature of a 0.900 kg aluminum pot…
A:
Q: An insulated, copper container has mass 200.0 g and holds 500.0 g of water. They are both initially…
A:
Q: A 3.50-g copper coin at 17.5°C drops 40.0 m to the ground. (a) Assuming 55.0% of the change in…
A: a) The expression to determine the energy required to raise the temperature of the coin is,…
Q: How much thermal energy is required to increase the temperature of a 390.00g sample of water from…
A: Given data: Mass (m) = 390.00 g = 390.00×10-3 kg Initial temperature (T0) = 15.00°C Final…
Q: A 2.5 kg lump of aluminum is heated to 96oC and then dropped into 9.0 kg of water at 5.1oC. Assuming…
A:
Q: A 70.0-kg block of ice at 0.00°C breaks off from a glacier, slides along the frictionless ice to the…
A: The objective of the question is to find out how much of the mass of the ice is melted by the…
Q: A 5.157 kg loose bag of soil falls from unknown height at a construction site. What is height in m…
A:
Q: One mole of water vapor at 346 K cools to 280 K. The heat given off by the cooling water vapor is…
A: Step 1: Step 2: Step 3: Step 4:
Q: A ceramic ball of radius 1.72 m and emissivity 0.900 is heated to 128°C. HINT (a) Convert the given…
A: Given data: theradius of a ceramic ball is emissivity is, temperature of a ball is, ambient…
Q: A coffee cup calorimeter contains 48.00 grams of water at 25.0°C. Two additional samples of water…
A: When heat energy is supplied to or absorbed from an object, according to the energy conservation…
Q: Find the total heat required (in kJ) to raise the temperature of a 0.5 kg of ice from −5.0°C to…
A:
Q: In a nuclear power plant, a 1.0 kg of water at 56.9 °C is converted into 1.0 kg of steam at 154.7…
A:
Q: 5. A 760 g piece of copper is heated in a furnace to a temperature T. The copper is then inserted…
A:
Q: Following vigorous exercise, the internal body temperature of a 72.5-kg person is 40.0°C. At what…
A: The amount of power in 30 min is,
Q: A cylinder containing an ideal gas a volume of 2.6 m^3 and a pressure of 1.5 x 10^5 Pa at a temp of…
A:
Q: You pour 998.00 cm3 of liquid mercury into a 1000.00 cm3-flask when both the mercury and the glass…
A: Given data The initial volume of the liquid mercury is: Vi-m = 998 cm3 The volume of the glass flask…
Q: A 95.0-kg block of ice at 0.00°C breaks off from a glacier, slides along the frictionless ice to the…
A:
Step by step
Solved in 2 steps with 2 images
- The American Burn Association states 3. You heat up an aluminum sphere of radius r, 1.27254 cm to 100 °C. You cool a 20.0 g copper ring to 0.00000 °C. The inner radius of the copper ring is r, 1.27000 cm. You then place the sphere on top of the ring and they are allowed to reach thermal equilibrium. Assume no heat loss to the surroundings. At the equilibrium temperature the sphere falls through the ring. (a) What is the thermal equilibrium temperature? (b) What was the amount of heat that was transferred between the ring and the sphere? (e) Which object lost the heat and which object gained the heat? (d) What is the mass of the aluminum sphere? Do not use the definition of density to solve for the mass. OTo treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 16.8 g, and its initial temperature is -10.7 °C. The water resulting from the melted ice reaches the temperature of his skin, 29.4 'C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table.Thank you!
- The same amount of heat entering identical masses of different substances produces different temperature changes. Calculate the final temperature when 1.70 kcal of heat enters 1.38 kg of the following, originally at 30.2°C. The specific heat capacity for each material is given in square brackets below. (a) water [1.00 kcal/(kg · °C)] °C (b) concrete [0.20 kcal/(kg · °C)] °C (c) steel [0.108 kcal/(kg · °C)] °C (d) mercury [0.0333 kcal/(kg · °C)] °CA 155 g copper bowl contains 230 g of water, both at 20.0°C. A very hot 300 g copper cylinder is dropped into the water, causing the water to boil, with 4.05 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy (in calories) is transferred to the water as heat? 8.6 X kcal (b) How much energy (in calories) is transferred to the bowl? 55 X kcal (c) What is the original temperature of the cylinder? 553.6 X °C Did you use the idea of conservation of energy? That is, did you equate the sum of the energy transfers to zero? For the bowl and cylinder, did you substitute the expression relating an energy transfer, the specific heat, the mass, and the temperature change? For the water, did you use the same expression to get the water to the boiling point? Did you also include an expression for the heat of vaporization? Did you use the given final temperature for each of the three materials?The same amount of heat entering identical masses of different substances produces different temperature changes. Calculate the final temperature when 1.40 kcal of heat enters 1.83 kg of the following, originally at 28.2°C. The specific heat capacity for each material is given in square brackets below. (a) water [1.00 kcal/(kg · °C)] °C (b) concrete [0.20 kcal/(kg · °C)] °C (c) steel [0.108 kcal/(kg · °C)] °C (d) mercury [0.0333 kcal/(kg · °C)] °C
- A 1 kg bar of copper is heated at atmo- spheric pressure of 1.013 x 105 N/m². If its temperature increases from 14°C to 54°C, find the work done by the copper. The linear expansion coefficient of copper is 1.7 x 10-5 (°C)¹, its density is 8920 kg/m³ and its specific heat is 387 J/kg. ° C. Answer in units of J. part 2 of 2 What quantity of thermal energy is trans- ferred to the copper in this process? The specific heat of copper is 387 J/kg.° C. Answer in units of J.A certain substance has a mass per mole of 41 g/mol. When 315 J is added as heat to a 33.0 g sample, the sample's temperature rises from 27.0°C to 41.0°C. What are the (a) specific heat and (b) molar specific heat of this substance? (c) How many moles are present? (a) Number Units (b) Number Units (c) Number UnitsSteam at 100°C is condensed into a 62.0 g brass calorimeter cup containing 220 g of water at 21.0°C. Determine the amount of steam (in g) needed for the system to reach a final temperature of 48.0°C. The specific heat of brass is 380 J/(kg · °C).
- I am stuck on this question i got for homework :( I got a final temperature as 150 degrees Celsius which not possibleA typical nuclear reactor generates 1000 MW of electric energy. In doing so, it produces “waste heat” at a rate of 2000 MW, and this heat must be removed from the reactor. Many reactors are sited next to large bodies of water so that they can use the water for cooling. Consider a reactor where the intakewater is at 18°C. State regulations limit the temperature of the output water to 30°C so as not to harm aquatic organisms. How many kilograms of cooling water have to be pumped through the reactor each minute?