How much energy in Joules (J) is needed to vaporize 15.0 g of rubbing alcohol?  The heat of vaporization of ethanol is 732.2 J/g.

Q: If 0.40 kJ of heat is removed from a sample of water and it cools from 25°C to 15°C, what is the…

A: Mass of water is approximately 9.57 grams

Q: 3.20 kJ of heat is required to raise the temperature of 37.0 g of magnesium from 45°C to 130°C. What…

A:

Q: How much heat must be absorbed by a 15.0-g sample of water to raise its temperature from 25.0 °C to…

A: The heat absorbed by the given system is determined by using following formula.

Q: How much heat ( in joules) does it take to heat 45.0 g of 23.0 C water until it is steam at 112.0 C?

A: Answer: Heat (in joule) = 117319.5 J

Q: Aluminum has a specific heat of ,0.902 J/g*K how much heat is lost when a piece of aluminum with a…

A: Given, the mass of aluminum =28.372 gspecific heat of aluminum =0.902 Jg.Kinitial temperature Ti…

Q: How much heat is released when 358 g of water cools from 68.3°C to 18.9°C? The specific heat of…

A: This is the question of thermodynamics Here we have to calculate heat released It uses the formula…

Q: How much heat in kJ is needed to raise the temperature of 130.0 g of water from 15 degrees Celsius…

A: Given, amount of water =130.0 ginitial temperature Ti =15 °Cfinal temperature Tf =100 °C ( boiling…

Q: The specific heat of copper metal is 0.385 J/g degree C. How much heat in Joules is necessary to…

A:

Q: Suppose you have samples of gold, iron, and aluminum, all of the same mass. If the same quantity of…

A: Given information, Specific heat of gold = 0.13 J/g °C Specific heat of iron = 0.45 J/g °C Specific…

Q: How much energy does it take to heat a cup of water (242 g) from room temperature (21.0°C) to its…

A: Step 1) Specific heat says that how much heat is required to raise that temperature 1 g of a sample…

Q: How much heat energy does 50.0 grams of water absorb if it’s temperature goes from 22.0 Celsius to…

A: Answer: Given data Mass of water m=50.0g Rise in temperature of water ∆T=(25.3-22)°C∆T=3.3°C

Q: How much heat, in joules and in calories, is required to heat a 28.4-g (1-oz) ice cube from −23.0 °C…

A: Given : Mass of ice cube = 28.4 g Initial temperature of ice cube = -23.0 oC And final temperature…

Q: How much heat is required to warm 162g of water by 33℃? Cwater = 4.184J/g℃

A: The amount of heat required to increase the temperature of one kilo gram of a substance by one…

Q: How much heat is gained by copper when 77.5 g of copper is warmed from 21.4°C to 75.1°C? The…

A:

Q: The same amount of heat is added to a 25-g sample of each of the following metals. If each of metals…

A: Given:: mass = 25 g Initial Temp. = 20.0 ℃ Which metal having highest temperature ?

Q: Determine the specific heat of 122 grams of an unknown substance if it absorbed 270 kJ of heat as it…

A: Specific heat of a substance can be defined as the amount of heat required to raise temperature by…

Q: 22.0 g of a metal absorbs 713 J when it is heated from 28.3 degrees to 72.8 degrees what is the…

A:

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: 1. A pure gold ring and pure silver ring have a total mass of 13.0 g. The two rings are heated to 62…

A: Given that: mass of silver + gold = 13.0 g initial temperature = 62.4 oC volume of water = 15.2 mL…

Q: A metal with a mass of 120 g absorbs 1800 J while undergoing a temperature change of 22 ∘C. What is…

A: Heat is defined as the form of energy which gives us the sensation of warmth. The relation between…

Q: Solid magnesium has a specific heat of 1.01 J/g°C. How much heat is given off by a 20.0 gram sample…

A: Given, Specific Heat, c= 1.01 J/g oC. Amount of Magnesium, m = 20 gram Temperature, T1 = 70.0 oC.…

Q: Mercury, with a freezing point of -38.8°C, is the only metal that is liquid at room temperature. How…

A: Given that,  Volume of mercury = 1.60 mL Mass of mercury m = density×volume          = 13.6 × 1.60 g…

Q: What is the final temperature when 5.0 g sample of brass initially at 25 degrees celsius absorbs 75…

A: Heat  is defined as thermal energy transferred between two systems at different temperatures coming…

Q: How much heat is released when the temperature of an 8.21 g sample of gold decreases from 87.9 oC to…

A: q = mc∆T  q is the amount of heat energy released or absorbed m is the mass of substance  c is the…

Q: A 224 g sample of gold at 18 °C absorbs 4830 J of heat upon heating. What is the final temperature…

A:

Q: The specific heat capacity of gold is 0.13 J/g°C. How many calories of energya needed to warm 0.513…

A: Q= cm∆T Q = energy given m is mass of substance ∆T is change in temperature. c is specific heat

Q: Copper has a specific heat of 0.382 J/g×°C. The temperature of an unknown mass of copper increases…

A: Specific heat is the amount of heat required to increase the temperature of one grams substance by…

Q: How many grams of water can be heated form 20.0°C to 45.0°C by the heat released from 215.0 g of…

A: Heat is the type of energy that is transmitted between two substances at different temperatures. The…

Q: A 22.4 g piece of an unknown metal loses 672 J of energy when it cools from 95.3°C to 28.5°C. What…

A:

Q: A 5.0-g sample of a metal increases in temperature from 20.0C to 22.0C when it absorbs 9.6 J of…

A:

Q: metal is heated from 25.0°C to 250.°C, and was found to have absorbed 878 J of energy as heat. What…

A: Heat flow from high temperature to low temperature.

Q: In a coffee cup calorimeter, 15.0 g sample of nickel metal is heated to exactly 100 °C and dropped…

A:

Q: 1. How much heat, in joules, is absorbed by 500.0 g of water as its temperature is increased from…

A: So we’ve to calculate the energy and specific heat capacity in the respective question. We can solve…

Q: The temperature of a sample of water increases from 20.0°C to 46.6°C as it absorbs 5650 J of heat.…

A: Given,  Initial temperature = Ti = 20.0 °C Final temperature = Tf = 46.6 °C Amount of heat absorbed…

Q: A 10.4 g sample of a liquid changes from 35.0 ºC to 25.0ºC upon removal of 85.0 J of heat. What is…

A: Given         Heat (Q)  = -85 Joule  Mass of sample  (m)      = 10.4 gram  Initial Temperature (T1…

Q: A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/degree C. What is the specific…

A:

Q: 3. If an ice cube (solid H2O) has a mass of 9.8 g, and it takes 334 J to melt 1 gram of solid H2O,…

A: Mass of ice cube = 9.8 g Mass of water= 150 g ∆T =( 75-35 )oC = 40oC

Q: A 25.0 g sample of lead, specific heat = 0.128 J/g  degrees Celcius , was warmed from 35.0 derees…

A: Heat absorbed by lead is calculated as follows,

Q: A 15.0 g piece of cadmium metal absorbs 134 J of heat as its temperature is increased from 24.0°C to…

A:

Q: 6.70 J heat is added to 5.71 g sample of unknown metal and temperature of metal increases by 0.798…

A: We know the equation of specific heat formula is: Q = m c Δ T where Q= heat energy (J) m= mass of…

Q: ) 100.0 g of 4.0°C water is heated until its temperature is 37°C. If the specific heat of water is…

A: Given datas ;  m = 100 g  Ti = 4°C  Tf = 37°C  c = 4.18 J/g.°C

Q: How much heat is gained by nickel when 213 g of nickel is warmed from 22.2 °C to 59.0 °C. J The…

A: Interpretation: Heat gained by nickel when 213 g of nickel is warmed from 22.2 oC to 59.0 oC is to…

Q: A blacksmith heats a 1,540 g iron horseshoe to a temperature of 1445°C before dropping it into 4,280…

A: Specific heat (s) is the heat required to raise the temperature by 1°C of the substance. It has the…

Q: The freezing point of mercury is -38.8 degrees Celsius. What Energy is released to the surroundings…

A: using the specific heat capacity and enthalpy of fusion to find the heat released.

Q: A student has two containers—one with 10 g of sand and one with 10 g of ethanol. (a) Which substance…

A: Given: 10 g of sand 10 g of ethanol The specific heat capacity of sand and ethanol is taken as…

Q: What is the specific heat of silver if it requires 86.3 J of energy to raise the temperature of 15.0…

A: According to thermodynamics, heat changed during a reaction is given by the relationship:q = mcΔT…

Q: How many degrees of temperature rise will occur when a 25.0 g block of aluminum absorbs 10.0 kJ of…

A: Specific heat (C) :-  The amount of heat required to raise the temperature of 1 gram of a substance…

Q: How much heat is required to warm a 4.1 lb Pyrex baking dish from 22 degrees C to 191 degrees C?

A:

Q: 19. You are taking a walk in the Arctic Circle and find a prehistoric person frozen in a block of…

A:

Q: TABLE 5.2 Specific Heat Values of Some Common Substances Substance Specific Heat (J/g °C) Substance…

A:

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.