How much heat (kJ) is needed to raise the temperature of 100.0 grams of water from 25.0°C to 50.0°C? O 1.05 O 10.5 O 0.598 10450 none of the above

Q: Suppose you burn a 2.3 g sample of potato chips. You use the heat given off from that process to…

A:

Q: Calculate the heat that must be supplied to a 500.0 g stainless steel vessel containing 450.0 g of…

A: The specific heat can be defined as the amount of heat per unit mass that is needed to raise the…

Q: 3. When a 70.5-g piece of an alloy is placed in 500 g of cold water in a calorimeter, the…

A: Here the heat absorbed by water to increase the Temperatures is released by the alloy whose…

Q: Suppose you heat a metal object with a mass of 34.4 g to 96.5 °C and transfer it to a calorimeter…

A: When the hot metal is dunked into the water, the heat is released by the metal and the equal heat is…

Q: A 25.0 g piece of metal at 4.0 °C is dropped into a calorimeter containing 13.6g of water.  The…

A: Heat lost by water = - Heat gained by metal                                          ...... (1)…

Q: If Water has a specific heat of 4.184 J/g°C. How much heat is required to increase 10.0 g of water…

A:

Q: Specific Heats of Substances Substance Specific Heat (J/g°C) Substance Specific Heat (J/g*C) Ice…

A: Answer

Q: In fertilizer, 15.0 g of urea (NH2 CONH2) is dissolved in 250 mL of water. A temperature change from…

A: Given that,  Amount of urea,  = 15.0 g Volume of water, m= 250 mL  = 250 g * density of water at…

Q: how many calories (cal) are equivalent to 7.25 kJ? (1 cal = 4.184 J )

A: Recall the relation between calorie and joule        1 cal=4.184 J We have to find the equivalents…

Q: 2. A lead pellet having a mass of 26.47 g at 89.98 °C was placed in a calorimeter containing 100.0…

A:

Q: What is the specific heat of a 41.5g piece of glass, if it takes 17.8 kJ of heat to raise its…

A: ∆H = mS∆T  ∆T = 68.5 - 20 = 48.5 °C

Q: Suppose you burn a 2.6 g sample of potato chips. You use the heat given off from that process to…

A: Given: The mass of the potato chips burned = 2.6 g The amount of water = 26.0 g The initial…

Q: The table lists the specific heat values of several substances. Substance Specific heat (cal/g.°C)…

A: Heat energy is given by q = m * C * ΔT where q = heat energy m = mass of the substance C = specific…

Q: If the specific heat of water is 4.186 J/g °C, how much heat is required to increase the temperature…

A:

Q: A student performs a calorimetry experiment. The student combines 100. g of 0.40 M HC1(aq) with 100.…

A: Heat absorbed by the particular species = mass × heat capacity × temperature change

Q: gnore lock

A: Specific heat capacity and heat are related by the following relation: Q=m×C×T Q= heat released m=…

Q: Which of the following will use the least amount of heat to increase in temperature by 10 °C? I. 2…

A: I. 2 g Zn (c = 0.387 J/g °C) II. 1 g Pb (c = 0.128 J/g °C) III. 2 g Au (c = 0.126 J/g °C) IV. 1 g…

Q: A substance weighing 14.2 g absorbs 65.03 J of heat, resulting in a temperature increase of 10.2 °C.…

A: The objective of the question is to identify the substance based on its specific heat capacity. The…

Q: A solution is made by mixing 212.0 mL of ethanol initially at 10.0 C with 212.0 mL of water…

A:

Q: What is the specific heat of 54.8 g of a substance that releases 445 Joules of heat upon cooling…

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

Q: The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the…

A: Below attached file showing the details answer All the best

Q: Help with these questions What is the specific heat of a metal sample if a 35 g sample absorbs 2.3 x…

A: Specific heat of a substance is defined as the amount of energy that is needed to raise the…

Q: How much heat is absorbed when the temperature of a 4.1 g copper coin increases from 15.3 °C 74.6…

A: The problem provides us with the following information:Mass of the copper coin (m) = 4.1 gInitial…

Q: . An amount of 125.0 gram of iron fibers has been heated from 39.0 °C to 127 °C. How much heat was…

A: Given data, Mass of Iron = 125.0 g Specific heat of iron  = 0.444 J/g ℃ Initia temperature (T1) =…

Q: A mug is said to hold 66.05 g of water at 14.59°C. A 103.86-g spoon at 61.96°C was placed in it,…

A:

Q: If 980 J of energy as heat are transferred to 6.2 L of water at 291 K, what will the final…

A: The amount of heat required to increases the temperature of the 1 g of the substance by 1 degree is…

Q: During an endothermic reaction in a beaker if we are part of the surroundings and touched the…

A: Given: The reaction is endothermic.

Q: A 4.77 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

A:

Q: 7. If you add a 120 °C platinum piece with a mass of 2.34 g (c = 0.126 J/g°C) to 100 g of 5.2 °C…

A:

Q: What is the specific heat of 20.0 g piece of an unknown substance that changes from 25°C to 75°C…

A: Heat required to raise the temperature of the substance through 1°C is known as specific heat of the…

Q: 1. What is the specific heat of ethyl alcohol if 129J of heat is required to raise the temperature…

A: Specific heat is defined as the heat required to raise the temperature of one gram of a substance by…

Q: 79.8 grams of a metal that is at temperature 92.39 oC is placed in 186.3 mL of water at 19.79 oC.…

A: Here use thermal equilibrium concept. Here final temperature is 24.68 degree celcius, So metal…

Q: 2

A: The heat in a calorimeter, qcal is given as : The heat change of a reaction in a calorimeter, qrxn…

Q: Calculate the temperature change when 7.52J of heat is released in a calorimeter having a heat…

A: Given,  Heat released = q = 7.52 J  Heat capacity of calorimeter = C = 470 J/°C  Temperature change…

Q: What will be the final temperature of a 552-g sample of water, initially at 14.0°C, after 584 kJ…

A: Given,  Mass of water, m = 552 g  Heat, q = 58.4 kJ = 58.4x103 J  Heat capacity of water, Cp = 4.184…

Q: A girl went to a tennis practise holding a bottle containing 2L (2 kg) of water in her sport bag.…

A: We have to predict the amount of heat absorbed by water.

Q: how much heat is required to raise the temperature of 5.0 g of aluminum from 25.0 c to 300.0 c

A: The objective of this question is to calculate the amount of heat required to raise the temperature…

Q: pecine heat capacity (J/g °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 water…

A:

Q: 105 mL of H2 O is initially at room temperature (22.0° C). A chilled steel rod at 2.0° C is placed…

A: The heat lost by water is given by  Q = mw Cw ΔTw  where mw = mass of water = density of water X…

Q: 8. 5820 g piece of copper is heated from 21.5°C to 322.3°C. Calculate the amount of heat absorbed in…

A: Step 1: Problem No. 8: Given data : mass (m)=5820g Change in temperatureΔT=Final temperature -…

Q: A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 90.0°C, determine the…

A:

Q: What will be the final temperature of a 814.4 g sample of water at 40.2°C if the sample gains 92.00…

A: "Since you have asked multiple question, we will solve the first question for you. If youwant any…

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.    

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.