calculate how much heat in kilojoules is absorbed by 948.0 g of liquid A in order for the temperature to increase from 20.00 degree celsius to 27.50 degree celsius? specific heat capacity of liquid A is 4.186 J/g degree celsius

Q: How much heat is emitted when 4.25  g  of water condenses at 25  ∘C ? The heat of vaporization of…

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Q: How much energy is released when 75.3 g of water vapor at 115 degrees C condense and cool to liquid…

A: We know ,energy released HH = m×S× ( tf − ti ) Where H = heat m = mass in gramsS=Specific Heat…

Q: Using the following data shown below for the heating curve and calculate the total amount of heat…

A: The specific heat capacity is defined as the amount of heat energy needed to raise the temperature…

Q: 3. What mass of water would need to evaporate from your skin in order to dissipate 1.7X10³ J of heat…

A: Given :  ∆Hvap = 2261 J/g  Heat given (q) = 1.7 x 105 J

Q: At a certain elavation, the boiling point of water is 98.5C. How much energy, in kilojoules, is…

A: Heat energy needed,Q= 11.0 KJ

Q: Use the information provided below to calculate the quantity of heat (in kJ) required to convert…

A: Given: Mass = 55.77g Molar mass= 29.3 g/mol Initial Temperature = 120.5°C Final Temperature = -…

Q: Why is the heat of vaporization of water greater at room temperature than it is at its boiling…

A: The heat of vaporization or heat of evaporation is the quantity of heat required by the compound or…

Q: How much energy is released when 35.0 g of water freezes? The heat of fusion for water is…

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Q: How many joules of heat are required to melt 4.5 g of copper at a temperature of 1083°C? Use the…

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Q: Carbon disulfide, CS2, is a colorless, toxic, highly volatile, and flammable liquid. What is the…

A: Given, CS2(l) ➝ CS2(g) ; ∆H° = ? ∆Hf°[CS2(l)] = 89.7 kJ/mol ∆Hf°[CS2(g)] = 116.9 kJ/mol Heat of…

Q: Explain why water in a swimming pool takes a long time to heat up at the beginning of the summer and…

A: Introduction: Specific heat is defined by the amount of heat needed to raise the temperature of 1…

Q: At a pressure of 1 atm, CO2 sublimes (changes directly from solid to gas) at -78°C. a. At 1 atm,…

A: Given :  Mass of CO2 = 2.20 gm  molar mass of CO2 = 44 gm/mol  Pressure  = 1 atm  Initial…

Q: Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the water…

A: Heat required to raise the temprature of water from 3.8°C to 36.6°C is given by , Q = ms∆T ,where m…

Q: How much heat is required to change  256.0 g  of water at  58.1 ° C  to steam at  100.0 ° C?

A: Given that: Mass of water, mwater = 256.0 g Initial temperature = 58.1⁰C Final temperature = 100.0⁰C…

Q: How much heat is required to change  266.4 g  of ice at 0 ° C to water at  0 ° C?

A: The mass of ice is = 266.4 g The temperature of ice is = 0oC The temperature of the water is = 0oC…

Q: Two 20.0 g ice cubes at -14.0 °C are placed into 265 g of water at 25.0 °C. Assuming no energy is…

A: Answer: This question is based on the principle of conservation of energy which suggests that heat…

Q: A coffee pot contains 310 grams of water at 100oC. How many calories of heat are required to…

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Q: How much energy (in kJ) is needed to heat 5.28 g of ice from -18oC to 30.0oC?  The heat of fusion of…

A: Given : Mass of ice = 5.28 g Initial temperature of ice = -18.0 oC Final temperature of water = 30.0…

Q: How much heat is required to vaporize 100.0 g of ethanol

A: Number of moles = mass ÷ molar mass  Molar mass of ethanol is 46.07 g/mol

Q: For a 7.48 gram sample of water at 0.63°C , what is the minimum amount of heat (in kJ) needed to…

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Q: Suppose 1.0 x 102 grams of ice absorbs 1255 J of heat, reaching a final temperature of -2.0°C.  What…

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Q: Three 15.0 g ice cubes at -28 C are placed in 350 g of water at 30 C. Assuming that no energy is…

A: Assuming the final temperature is T degree Celsius and is greater than 0. Since the heat required in…

Q: How much heat is needed to convert 0.232 grams of ice into steam, from -32.5 degrees C to 112…

A: Heating cold ice to hot steam requires Five distinct steps : 1. Heat -32.50C ice to 00C ice  2. Melt…

Q: How much heat is required to vaporize 2.31 mol of methane, CH¼, at its boiling point? The heat of…

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Q: Use the information provided below to calculate the quantity of heat (in kJ) required to convert…

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Q: How much heat is needed to convert 35.6g of ice at 0°C to water at 27°C? AHfus of ice = 6.01 kJ/mol…

A: Heat required = Raise the temperature from 0 oC to 27 oC  Q = mc delta T

Q: The heat of fusion of acetic acid, the principal organic component of vinegar, is 192 J/g. How much…

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Q: A heating curve of one gram of a pure solid at 1 atm is shown to the right. Which factor affects the…

A: A pure solid is heated. In the given heating curve, Segment AB represents all solid (heat is…

Q: A 193.1 g sample of water at 21.2°C is heated to steam at 131.5°C. How much heat was absorbed?

A:

Q: Two 20.0 g ice cubes at −16.0 ∘C−16.0 ∘C are placed into 255 g255 g of water at 25.0 ∘C.25.0 ∘C.…

A: Given data:

Q: How much energy is required to melt 553 g553 g of ice into liquid water at 0 degrees Celsius? 0…

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Q: The heat of fusion for sea ice is 79.70 cal/g. How many calories of heat are needed to melt a 35.00…

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Q: How much energy is absorbed or released when 2.30 moles of water (4.184 J/g°C) cools from its normal…

A: Given: Moles of water = 2.30 moles. Specific heat capacity of water = 4.184 J/g C∘. We have to find…

Q: 11. Based on the heating graph shown in the figure for a substance, X, at constant pressure, Energy…

A: 11.a) Heat transfer     = mass × temperature change × specific heat  Or,  Q = m × T × S  Or,   T =…

Q: A quantity of ice at 0 °C was added to 64.3 g of water in a glass at 55 °C. The final temperature of…

A: Given,Mass of water = 64.3g. Temperature of water = 550C.Final temperature of system = 150C.Heat of…

Q: Which of the following does NOT represent a step on the heating curve of water?

A:

Q: Consider the heating curve for 1.00 mole of an unknown substance as it is heated from a solid to a…

A: We are having an heating curve of substance, we have to predict line having both solid and liquid…

Q: How much heat (kJ) is absorbed by 948.0 g of water in order for the temperature to increase from…

A: Specific heat: The amount of heat energy required to raise the temperature of one gram of a…

Q: If the following solid metals all have the same mass, which will undergo the largest temperature…

A:

Q: How much heat is required to convert 135 g of ice at −15 °C into water vapor at 120 °C?

A: heat required is calculated by,q=m c ⊿Twhere,m=mass of samplec=specific heat of substance ⊿T=the…

Q: How much energy is required to melt 553 g553 g of ice into liquid water at 0 ∘C?0 ∘C? The heat of…

A: Total energy required= mXL m= mass of ice = 553g L=heat of fusion= 333.6 J/g

Q: How much energy is required to melt 357 g of ice into liquid water at 0 °C? The heat of fusion for…

A: We can answer this question using the equation, Q = Lice × m Q is  the amount of heat required to…

Q: Two 20.0 g ice cubes at −13.0 ∘C are placed into 285 g of water at 25.0 ∘C. Assuming no energy is…

A:

Q: Use the information provided below to calculate the quantity of heat (in kJ) required to convert…

A: Given the mass of the substance = 63.01 g Molar mass of the substance = 27.1 g/mol => moles of…

Q: Determine the heat in kJ to heat 7.18 moles of ice from -29.286 degrees celcius to -2.357 degrees…

A: Mass can be determined using the below given equation,

Q: How much heat will it take to raise the temperature of 10 g of ice from −30°C to −20°C?   The…

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Q: How much energy must be supplied to convert 125g of ice at 0 degrees celcius to 125g of water at 91…

A: We will be using two types of heat in the whole process:   Q1  = Heat required to convert the ice at…

Q: Calculate the heat change in joules for vaporization of 9.00 g of water at 100 ∘C.

A: Heat of vaporisation of water is 2256 J/g/0C.Thus, when 1 mol ( 18 g) of water is vaporised, 2256…

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.