Calculate the heat of vaporization for a liquid in J/g. When it absorb 53,760 J joules of energy to change 40.0 g of the liquid to vapor at the boiling point? O 1344 J/g O 13.44 J/g 1.344 J/g O 134.4 J/g

Q: Calculate the heat required to vaporize 102 g of water at a temperature of 100oC   if the Heat of…

A: The process of conversion of a substance in its liquid state into its gaseous state is called…

Q: 18) Ethyl chloride, C2H5C1, is used as a local anesthetic. It works by cooling tissue as it…

A: It is based on the concept of thermochemistry. Here we are required to find the heat that could be…

Q: Compound Z has a heat of vaporization of 155.9 J/g, a specific heat capacity of 2.08 J/gºC, and…

A: Given, Boiling point = 72.1 °c □Hvap = 155.9 J/g C(l) =  2.08 J/g-°c Mass of. Z(m) = 562.4 g

Q: How much energy is needed to boil 45.0g of water at its boiling point? Water's heat of vaporization…

A: Given: Mass of water = 45.0 g. And heat of vaporization of water = 40.65 KJ/mol.

Q: Benzene has a boiling point of 80.1 °C, and a specific heat capacity of 1.8 J/g °C in the liquid…

A: we have to calculate the heat released when benzene is cooled from 114 degree C to 55.1 degree C

Q: How much energy (heat) is required to convert 33.5 g of H2O(l) at 8.7°C to H2O(g) at 129.3°C?…

A: Mass of water (liquid)  = 33.5 gMoles of H2O =  = 1.86 molInitial temperature (T1) = 8.7 °CFinal…

Q: The following information is given for silicon at 1 atm: Heat of vaporization = 2.528 × 103 cal/g…

A: Given : Mass of silicon = 44.90 g Initial phase of silicon = solid…

Q: Which processes absorb heat? vaporizing 65.0 mL of water freezing 12.5 g of water condensing 90.0 mL…

A: When solid changes to liquid or gas, it will require energy, and hence heat is absorbed.  When a…

Q: Determine the amount of heat required to convert 65.25 g of solid Ca at 651°C into liquid Ca at…

A: Answer :

Q: A sample of C₃H₄Br₂ has a normal boiling temperature of 131.5 °C. The enthalpy of vaporization for…

A: The heat required to change the temperature form T1= 97.5 °C…

Q: A pressure cooker (InstaPot) works by increasing the temperature that water in food or cooking food…

A:

Q: How much energy is removed when 45 grams of ethanol condenses to liquid? Ethanol heat of…

A: Given : Mass of ethanol condensed = 45 g Molar mass of ethanol = 46 g/mol. And heat of vaporisation…

Q: 4. You have a beaker of water at 25 C, that has a mass of 145.5g. How much energy is needed to…

A:

Q: The graph shows a heat curve for an unidentified substance discovered by the Mars rover. What is…

A: We can determine Fusion temperature ( melting or freezing point ) and vaporization temperature from…

Q: What will the final temperature (in be if you add 400 kJ of heat to 1.00 L of water at 20 °C? The…

A: When heat is given to water, the temperature of water will increase.this increase in temperature is…

Q: How much energy is needed to change the temperature of 39 g of water from 10.0 °C to 95.0 °C?

A: Since water remains in liquid form from 10°C to 95°C . Heat required, Q = mcp(l) ∆T ,where m is the…

Q: Consider the following selected properties of water: 1.00 g/mL Density (liquid water): d = Heat of…

A: As we needed the amount of heat that is required to vaporize 54 mL of water, we only need the data…

Q: For a given species, see the thermodynamic values below. Boiling Point: Melting Point: Heat of…

A: The quantity of heat energy absorbed or released in a chemical reaction can be calculated using the…

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

A:

Q: Calculate the amount of energy needed to change 10 g of solid mercury at its melting point to…

A:

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 energy (heat) is required to convert 26.1 g of H2O(l) at 32.5°C to H2O(g) at 119.2°C?…

A: Given mass of water ice, m = 26.1 g Molar mass of water = 18.02 g/ mol Therefore,moles of water =…

Q: the vapor pressure of water at 25 C is 3.13 x 10^-2 atm, and the heat of vaporization of water is 25…

A:

Q: Calculate the heat absorbed when 134.7 g of ice is heated from -19.8oC to 135.2oC.  Specific heat of…

A: The formula to calculate the heat absorbed (q) is given by q = m * c * ΔT, where m is the mass, c is…

Q: Suppose that 117.2 J of heat energy is required to completely vaporize 4.3 g of a pure liquid. If…

A:

Q: How much energy in Joules (J) is needed to vaporize 15.0 g of rubbing alcohol?  The heat of…

A: The amount of heat energy required to vaporize the 15.0 g of rubbing alcohol is to be determined.…

Q: Given that the heat of vaporization of water is 2256.4 kJ/kg, how much energy (kJ) does it take to…

A:

Q: How much heat is released ( in J) when 54.0 g of water at 10.0 °C is cooled to form ice at - 10.0…

A: Given the mass of water, m = 54.0 g  The initial state is water at 10.0 oC.  The final state is ice…

Q: Calculate heating ice from -10. To 0.0C. Using the information below: What is the heat in Joules…

A: What is the heat in Joules required to convert 25g of -10.C ice into 150C steam? Given data : Heat…

Q: How much heat energy is required to convert 90.2 g of solid iron at 24 C to liquid iron at 1538 ∘C?…

A:

Q: Consider the following selected properties of water: Density (liquid water): d = 1.00 g/mL Heat of…

A:

Q: A mass of 100 g of a liquid at 25 oC is heated to raise its temperature to 50.0 oC. The thermal…

A: Specific heat (S) :-  The amount heat needed to rise the temperature of one gram of a substance…

Q: The following information is given for lead at 1 atm: boiling point = 1.740×103 °C Hvap(1.740×103…

A: Given that : For lead : boiling point = 1.740×103 °C Hvap(1.740×103 °C) = 858.2 J/g melting…

Q: A 45.0 g chunk of ice at -12°C absorbs 12.0 kJ of heat. How many grams of ice melt? sp heat of ice…

A: Ice is at -12°C and it can not melt at this temprature For ice to melt temperature should be 0°C…

Q: Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of…

A:

Q: Ethanol (C₂H5OH) melts at -114 °C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02…

A:

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: Use the information provided to calculate the quantity of heat (in kJ) required to convert 59.22 g…

A:

Q: a. Calculate the heat required to melt 7.64 g of benzerie at jts normal melting point. Heat of…

A: Given: Mass of benzene = 7.64 g. Heat of fusion of benzene = 9.92 KJ/mol. And heat of vaporization…

Q: 13. Calculate the heat absorbed when 27.45 g of ice is heated from -30.00°C to 120.0°C. Specific…

A: Given: mass of ice , m= 27.45g  initial temperature, T1=-30∘C  final temperature, T2=120∘C

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.