When you put the iron cube in the olive oil and the brick cube in the water what loses heat more quickly and why? The oil or the water? Explanation why oil or water.

Q: A student is using calorimetry to determine the heat of solution for various salts. When the student…

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Q: 4. What mass of water would absorb 7.00 × 10² cal of heat if the temperature is increased from…

A: Heat of a reaction is defined as the heat  produces or absorbed during the reaction which can be…

Q: A 500-g piece of metal (a steel) is dropped into 775 mL of water at 23.5 °C. The final temperature…

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Q: 3. When 2.0 g of NaOH is the heat of dissolution are dissolved in 49.0 g of water, the temperature…

A: 3.) First we need to calculate the heat using the formula Q = mC∆T  Then we need to calculate moles…

Q: Because water has such a hyh specific heat capacity, it heats and cools more slowly than land. How…

A: Water has a high specific heat capacity which means that water needs more energy to raise its…

Q: A calorimeter is pictured below. When substances are dissolved in water, they can absorb or release…

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Q: How much will the temperature of a cup (183 g) of coffee at 96.1 °C be reduced (in °C) when a 45 g…

A: The problem is asking us to find the final temperature of the coffee after a silver spoon is placed…

Q: The specific heat of a substance is the amount of heat required to raise the temperature of one gram…

A: Given --> Q = 357 J  S = 0.362 J/g°C T1 = 24.1°C T2 = 80.6°C

Q: If 63.50 g of an unknown metal at 97.6 °C initially produced a resulting temperature of 39.5 °C when…

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

Q: What happens when Ethanol burns and what happens after it burns? What happens to the matter in…

A: Ethanol is a chemical substance made up of carbon, hydrogen and oxygen atoms. The chemical formula…

Q: How much will the temperature of a cup (175 g) of coffee at 94.3 °C be reduced (in °C) when a 47 g…

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Q: 4

A: The specific heat required to raise the temperature of per gram of a substance is given as:   The…

Q: A 0.562 g sample of KCl is added to 35.8 g of water in a calorimeter. If the temperature decreases…

A: The heat capacity of the resulting solution is 4.18 J/goC, which states that 4.18 J of energy will…

Q: How much will the temperature of a cup (176 g) of coffee at 94.8 °C be reduced (in °C) when a 45 g…

A: Given, mass of cup of coffee,mc = 176 g initial temperature of cup , Tc=94.8°C mass of silver spoon…

Q: 1. How much heat must be added to a 38-g sample of aluminum to increase its temperature by 250.0°C?…

A: Dear student since you have posted multiple questions, As per BARTLEBY QnA guidelines we are allowed…

Q: 4. How much will the temperature of a cup (180 g) of coffee at 95 °C be reduced when a spoon…

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Q: If two objects, A and B, of different temperature come into direct contact, what is the relationship…

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Q: sample of sodium hydroxide dissolved in water, releasing heat to the surrounding water, and causing…

A: According to first law of thermodynmics, the total energy of a system remains constant.if one…

Q: Baked pizza dough has a heat capacity of 2.1 J/g C pizza sauce, which is mostly water, had a heat…

A: The objective of the question is to understand the concept of heat capacity and how it affects the…

Q: How much heat is released when 8.00 grams of solid magnesium react with gaseous oxygen to produce…

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Q: You place a piece of unknown metal in the oven and heat it to 185°C.  You then place the metal into…

A: Given: Mass of metal = 346 g. Volume of water = 250 mL. Initial temperature of water = 24.1 oC Final…

Q: .  A 70.0-g piece of metal at 80.0 °C is placed in 100 g of water at 22.0 °C contained in a…

A: When a hot metal is placed in cold water, water gains heat energy and metal loses heat energy.

Q: When hydrogen and oxygen are burned to produce water, heat is produced at the rate of 58 kcal/mole…

A: Given: Heat produced per mole of water = 58 Kcal/mol of water. And 1 mole of water contains = 6.02 ×…

Q: student is asked to determine the heat of solution in J/g for the compound ammonium nitrate…

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Q: Section 7: Heat 1. When ice melts, describe what happens to the energy of the air around it. 2.…

A: Heat absorption depends on heat capacity of substance.

Q: How many kilojoules of heat will raise the temperature of 1.50 kg of water from 22.00°C to 25.00°C?

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Q: The answer to this question is a numerical answer. Please report the numerical answer to 1 decimal…

A: Given:  The volume of HCl is 50.0 mL. The volume of NaOH is 31.8 mL. The molarity of HCl is 0.100 M.…

Q: A solution is made by mixing 197.3 g of ethanol initially at 10.5°C with 250.0 g of water initially…

A: We know that, according to the law of conservation of heat energy, energy gained or loss by the…

Q: In a calorimetric analysis, 2.42 g of potassium chloride is weighed. The heat of solution of this…

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Q: For this question, you are trying to determine which beaker will have more heat absorbed and why.…

A: Answer:- This question is answered by using the simple concept of calculation of heat absorbed by…

Q: Is dissolving AgNO3 in water an exothermic or endothermic process? What about dissolving MgSO4 in…

A: A chemical reaction in which heat energy is released is called exothermic reaction. Enthalpy is…

Q: the heat released for a complete reaction of 1 mole of carbon to 1 mole of carbon dioxide is 393kj.…

A: Given,  Given moles of carbon = 1 mole  Moles of CO2 = 1 mole  Amount of heat releases = 393 KJ…

Q: Part A You can bring only one into your sleeping bag. Which one should you choose to keep you…

A: The specific heat capacity of Aluminium is 900 J/kg°C but for water, it is 4,200 J/kg°C. Specific…

Q: A reaction between Mg and aqueous hydrochloric acid was performed to determine the heat of the…

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Q: A cold pack contains 134.4 g of water and 40.7 g of ammonium nitrate. What will be the final…

A: The formula which is used in the solution is shown below. Q = mcΔT ⇒ ΔT = Q/mc

Q: In a few sentences, relate these energy diagrams (the amount of energy absorbed by hot versus cold…

A: Energy diagrams generally represent the amount of energy required to raise the temperature of a…

Q: reach

A: Heat(Q) = mass • specific heat capacity • ∆T  Mass = 91.2g  Specific heat capacity of water =…

Q: 4. The specific heat of water is quite high at 4.184 J/gC. Explain how life on this planet would be…

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

Q: To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of…

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Q: If you added 35.5 ml of an HCI solution to 35.5 ml of an NaOH solution and the temperature increased…

A: Given: Volume of HCl solution = 35.5 mL Volume of NaOH solution = 35.5 mL Initial temperature of…

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.