If you combine 270.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture Use 1.00 g/mL as the density of water. Tinal = °C

Q: If you combine 260.0 mL of water at 25.00 °C and 130.0 mL of water at 95.00 °C, what is the final…

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Q: e final temperature of th

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Q: solution is made by mixing 260.0 mL of ethanol initially at 12.5 °C with 260.0 mL of water initially…

A: According to Law of calorimetry,amount of heat released by the substance having higher temperature…

Q: If you combine 360.0 mL of water at 25.00 °C and 140.0 mL of water at 95.00 °C, what is the final…

A: We know that, according to the law of conservation of heat energy, heat lost by hot water sample is…

Q: If 980 calories of energy as heat are transferred to 62.85 grams of a substance with an initial…

A: The amount ot heat is required to raise the temperature of body of unit mass to one degree Celsius…

Q: A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains…

A: Given, mass of the water (m) =7.30 kg = 7300 gInitial temperature T1=30.8 0C= 273K +30.8 =…

Q: Suppose it is winter and the system is filled with methanol. The density of methanol is 0.80 g/cm3.…

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Q: Specific Heats of Substances Substance Specific Heat (cal/g⋅°C) Brick 0.20 Ethanol 0.58…

A: The concept is based upon specific heat capacity which may be defined as the amount of heat energy…

Q: If 44.8 kJ of heat were added to 166 g of liquid water (specific heat of 4.184 J/g °C) at 18 °C, how…

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Q: In joules, how much heat is released when 42.0 g of Ag cools from 182. degrees C to 126. degrees C?…

A: We have to find out the heat release when 42 g Ag is cool. Given :  mass of Ag = m =42 g Initial…

Q: If you combine 400.0 mL of water at 25.00 °C and 130.0 mL of water at 95.00 °C, what is the final…

A: This numerical will be solved using the heat equilibrium formula that is given as:…

Q: If you combine 300.0 mL of water at 25.00 °C and 110.0 mL of water at 95.00 °C, what is the final…

A: When we mix the hot and cold water, the heat lost by hot water Q1 will be equal to the heat gained…

Q: Determine the final temperature of a 32.3 mL salt solution initially at 21.05ºC when 1.93 kJ of heat…

A: Volume of solution(V) = 32.3 mL Density of solution(d) = 1.235 g/mL Mass = V × d   = 32.3 × 1.235 =…

Q: If 132 g of ice at 0.0°C is added to 1.64 L of water at 98°C, what is the final temperature of the…

A: a) Given: Mass of ice = 132 g. Initial temperature of ice = 0.0 oC Volume of water = 1.64 L = 1640…

Q: If 2.500KJ of heat are added to 50.0g of water at 25.00 °C, what would be the final temperature of…

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Q: How many kJ of heat are needed to raise the temperature of 10.0kg of liquid water from 24 6 °C to 46…

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Q: A solution is made by mixing 260.0 mL of ethanol initially at 15.5 °C with 260.0 mL of water…

A: Given volume ethanol =260.0 mLinitial temperature of ethanol =15.5 °Cdensity of ethanol =0.789…

Q: How much heat, in calories, must be added to a 102.0g iron block with a specific heat of 0.449 J/g…

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Q: If you combine 310.0 mL of water at 25.00 °C and 140.0 mL of water at 95.00 °C, what is the final…

A: Given :-  First volume = 310.0 mL  First Temperature = 25.00°C  Second volume  = 140.0 mL  Second…

Q: Calculate the final temperature that results when A 12.6 g sample of water at 22.9 0C absorbs 875 J…

A: The given two problem can be solved by this equationQ=m.c.△TWhereQ=Amount of heat absorbed or lost…

Q: 3. A blacksmith heated an iron bar to 1445°C. The blacksmith then tempered the metal by dropping it…

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Q: 20.0 g of a solid substance X initially at 25.0 °C is heat to its melting point at 65.0 °C. Heat is…

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Q: Coffee cup calorimetry was used to determine the enthalpy of solution of lithium iodide (LiI): A)…

A: We'll answer the first question, since the amount of  solid lithium iodide is not given in the…

Q: 1.09 kcal of energy is added to 45 grams of water at an initial temperature of 23.4°C. What is the…

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Q: If you combine 370.0 mL of water at 25.00 °C and 130.0 mL of water at 95.00 °C, what is the final…

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Q: A 234.66 gram aqueous solution has a specific heat of 4.186 J/gºC. The solution is at 28.1 °C. What…

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Q: If you combine 270.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final…

A: By energy conservation: Let final temperature = Tf oC Heat loss by hot water = heat gain by cold…

Q: Metal Specific Heat (J/goC) Calcium 0.647 Iron 0.449 Silver 0.235 Gold 0.129 In joules,…

A: Mass of Ag(m) = 44.0g  Initial temperature (T1) = 189°C Final temperature (T2) = 129°C

Q: One beaker contains 156 g of water at 20. °C, and a second beaker contains 76.8 g of water at 95 °C.…

A: Heat gained (QGained) and heat lost (QLost) is calculated as shown in equation (1) and (2)…

Q: ) 4.184 J g-1 °C-1 × 114.9 × 103 mg × (32.60 °C – 11.8 °C) = ______________

A: Given, 114.9×103 mg = 114.9×103×10-3 g.  (32.60-11.8)°C = 20.8°C

Q: 14.0 g of cream at 20.3 °C are added to an insulated cup containing 100.0 g of coffee at 78.8 °C.…

A: Given that 14.0 g cream at 20.3 °C are added to an insulated cup containing 100.0 g of coffee at…

Q: when 20 grams of salt is dissolved in 95 grams of water, the temperature of the solution decreases…

A: When the solute is dissolved in the solution and the amount of heat released is known as the heat of…

Q: heat change of the reaction Al2Cl6(s) + 6 Na(s) ⎯→ 2Al(s) + 6 NaCl(s) is –256.2 kcal.  The heat of…

A: Given, □Hrxn = -256.2 kcal □Hf(NaCl) = -98.3 kcal □Hf(Al) = Hf(Na) = 0 kcal ( in standard state…

Q: If you combine 360.0 mL of water at 25.00 °C and 130.0 mL of water at 95.00 °C, what is the final…

A: We have to calculate the final temperature of mixture