Q: If 161 g of water has 5.72 X 10 4 J of heat added to it, what is the change in temperature?
A: We have to use the formula: q = mc ΔT where q = heat added/ removed that is 5.72 X 10 4 J…
Q: What is specific heat ? O The study of heat changes that accompany chemical reactions and phase…
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Q: Calculate
A: Water is not heated upto 100°C so it is not boiled. So that, specific heat capacity of water is…
Q: Calculate the amount of heat in joules needed to increase the temperature of 350 g of water from 20…
A: Specific heat capacity is amount of heat needed to increase the temperature of one gram of substance…
Q: A sample of water at 23.9 °C required an input of 2.68 × 104 J of heat to reach its boiling point,…
A: Required heat is calculated by using below formula,
Q: How much heat must a 30.0 g sample of water absorb to raise its temperature from 22.0 ∘C to 67.0 ∘C?…
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Q: Calculate the heat capacity, in joules per degree, of 28.4 g of water. Specific heat of water is…
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Q: q= 4.184 heat energy in joules. Use the formula: q=(m)(c)(ΔT) where m=mass of water being heated in…
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Q: If 44.8 kJ of heat were added to 166 g of liquid water (specific heat of 4.184 J/g °C) at 18 °C, how…
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Q: What mass of water can be heated from 10.0 °C to 75.0 °C using 95.1 kJ of heat?
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Q: How much heat is released when 60.5 grams of water at 60.0 degrees C changes to water at 12.5…
A: The question is about calculating the amount of heat released when 60.5 grams of Water at 60oC…
Q: How much heat, in joules and in calories, must be added to a 75.0–g iron block with a specific heat…
A: Heat is the transfer of energy due to the difference in temperature.
Q: Explain how the high specific heat capacity of water can affect the weather in coastal regions.
A: Specific heat capacity is the amount of heat change in bringing one degree (Celsius or Kelvin)…
Q: What is the volume of glucose, C6H12O6, that must be burned to release 1.00 x 103 kJ of heat? (C:…
A: Given data, Density of glucose = 1.54g/cm3 ∆H for glucose = 132kJ/mol Energy required = 1.00 x 103kJ…
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: 4. If 5.524 x 10°J of heat is applied to a 702.1 g sample of iron, by how many degrees Celsius will…
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Q: What quantity of heat energy (in Joules) is required to raise the temperature of 454g of tin from…
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Q: The evaporation of water is endothermic: H2O(l) + 44.01 kJ --------> H2O(g) If…
A: To find mass of water that will evaporate.
Q: How much heat (in kilojoules) is gained by 231 grams of water that is warmed from 25.00C to 39.00C?…
A: Given: Mass of water=231 g Temperature change, ∆T=(39.0-25.0)°C=14 °C The heat gained q =? kJ…
Q: Determine the amount of heat energy in joules required to raise the temperature of 7.40g of water…
A: Given: Mass of water = 7.40 g Initial temperature = 29°C Final temperature = 46°C Standard data:…
Q: A 50.0g sample of Fe at 100 °C is added to 500.0 mL of water at 35 °C in a perfectly insulated…
A: A 50.0g sample of Fe at 100 °C is added to 500.0 mL of water at 35 °C in a perfectly insulated…
Q: 9. If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature…
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Q: How many joules of heat are absorbed when 1000g of water is heated from 18oC to 85oC? The specific…
A: We have to find how many joules of heat are absorbed when 1000g of water is heated from 18oC to…
Q: Question 88
A: When 47.5 J of heat are added to 13.2 g of a liquid, its temperature rises by 1.72 °C. The heat…
Q: Calculate the amount of heat absorbed by 100 g of water that warms from 100 K to 273 K.
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Q: A sample of water at 15.6 °C required an input of 2.55 × 104 J of heat to reach its boiling point,…
A: We know that q = m × C × (Tfinal - Tinitial ) Where q = heat input m = mass of reactant, water C =…
Q: Calculate the quantity of heat (in Joules) required to raise the temperature of 20.0 g of water from…
A: Given that : Maas of water (m) = 20.0 g Initial temperature Ti = 25.1°C Final temperature Tf =…
Q: you apply 37.0 kj of heat energy to 155 grams of water 25 celsius. does the water boil? if not what…
A: Given: mass of water, m = 155g heat supplied to water, ∆H=37.0KJ…
Q: Calculate the heat lost by the liquid water (in kJ).
A: The equation of heat is as follows : q = m × c × ∆T…
Q: How much heat, in joules, must be added to a 95.8 g iron block with a specific heat of 0.509 J/g °C…
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Q: How many kilojoules of heat are absorbed when 2.00 L of water is heated from 12.5°C to 93.5°C?
A: Mass= density×volume Mass= 1×0.002=0.002gm Now Q=mc∆T Q= 0.002×4.18×(93.5-12.5) Q= 0.067×10-6kj
Q: How much heat is required to warm 1.50 kg of sand from 25.0 °C to 100.0 °C?
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Q: 50 g of copper is heated to increase its temperature by 10° C. If the same quantity of heat is given…
A: Given: The mass of copper (Cu) is 50 g The increase in temperature of copper is 10oC The mass of…
Q: If the temperature of a 500.0 -g sample of liquid water is raised 2.00 celsius, how much heat is…
A: We have to Given : m = 500.0 g Raised in…
Q: What mass of water will change its temperature by 3.00 degrees C when 525 J of heat is added to it?
A: The answer to the following question is-
Q: How much heat (in kilojoules) is gained by 294 grams of water that is warmed from 25.00C to 57.00C?…
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Q: How much heat must a 22.0 g sample of water absorb to raise its temperature from 21.0 ∘C to 75.0 ∘C?
A: The specific heat can be defined as the amount of heat per unit mass that is needed to raise the…
Q: Measuring the change in temperature versus time upon addition of a hot metal specimen to 10.3 mL of…
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Q: A quantity of water is heated from 25.0 Degrees Celsius to 36.4 Degrees Celsius by absorbing 325…
A: Specific heat :- The amount of heat required to raise the temperature of 1 gram of a substance…
Q: What quantity of heat is required to raise the temperature of 55.0 g of gold from 32 degree Celsius…
A: Heat required to raise the temperature of solids is given by Q = mCΔT where m = mass C = specific…
Q: How much heat, in joules (J), must be added to a 75.0-g iron block with a specific heat of 0.449 J/g…
A: Given: Mass of iron block =75.0 g Specific heat of iron =0.449 J/g oC Initial temperature(T1) =25 oC…
Q: If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?
A: The increase in temperature of a substance with respect to the quantity of heat transferred depends…
Q: How much heat must be absorbed by 375 grams of water to raise its temperature by 25° C? Specific…
A: Given, mass = 375 g Specific heat, c = 4.184 J/g°C Heat = ?
Q: Calculate the quantity of heat required to warm 1.25 L of water from 22.0°C to 98.0°C in an electric…
A: We have 1.25 L of water , initial and final temperature are 22°C and 98°C, we have to calculate the…
Q: Determine the amount of heat required to raise 10 grams of water 5 degree celcius ?
A: Specific heat capacity of water = 4.18 J/g oC
Q: The specific heat of water is 4.184J/g°c. How many joules of heat will be removed from 2.00g of…
A: The amount of heat absorbed or released is related to specific heat capacity as,…
Q: Define the specific heat capacity of water. What units are used for this value? How much heat is…
A: 1. Solution - Specific heat is defined by the amount of heat needed to raise the temperature of 1…
Q: If 57600 J of energy were absorbed by 250. g of water at 0.0 ̊C, what would be the final…
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A sample of water at 16.0 °C required an input of 1.97 × 104 J of heat to reach its boiling point, 100.0 °C. What was the mass of the water?
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