What is the final temperature in a squeezed cold pack that contains 41.5 g of NH4NO3 dissolved in...
What is the final temperature in a squeezed cold pack that contains 41.5 g of NH4NO3 dissolved in 125 mL of water? Assume a specific heat of 4.18J/(g⋅∘C) for the solution, an initial temperature of 25.5 ∘C, and no heat transfer between the cold pack and the environment.
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What is the final temperature in a squeezed cold pack that contains 41.5 g of NH4NO3 dissolved in...
Instant cold packs used to treat athletic injuries contain solid NH4NO3 and a pouch of water....
Instant cold packs used to treat athletic injuries contain solid NH4NO3 and a pouch of water. When the pack is squeezed, the pouch breaks and the solid dissolves, lowering the temperature because of the endothermic reaction NH4NO3(s)+H2O(l)→NH4NO3(aq) ΔH= +25.7 kJ. What is the final temperature in a squeezed cold pack that contains 43.5 g of NH4NO3 dissolved in 125 mL of water? Assume a specific heat of 4.18J/(g⋅∘C) for the solution, an initial temperature of 29.0 ∘C, and no heat...
Instant hot packs contain a solid and a pouch of water. When the pack is squeezed, the pouch breaks and the solid dissolves, increasing the temperature because of the exothermic reaction. The followin...
Instant hot packs contain a solid and a pouch of water. When the pack is squeezed, the pouch breaks and the solid dissolves, increasing the temperature because of the exothermic reaction. The following reaction is used to make a hot pack: LiCl(s)⟶Li+(aq)+Cl−(aq)ΔH=−36.9kJ What is the final temperature in a squeezed hot pack that contains 20.3 g of LiCl dissolved in 112 mL of water? Assume a specific heat of 4.18 J/(g⋅∘C)for the solution, an initial temperature of 25.0 ∘C, and...
10) (10pts) A cold pack consists of a small inner bag that contains water inside another...
10) (10pts) A cold pack consists of a small inner bag that contains water inside another larger bag that contains solid ammonium nitrate. When a cold pack is needed, the inner bag is broken and the water and ammonium nitrate are shaken together to dissolve the solid. If the inner bag contains 117 mL of water (density 1.00 g/mL), how many grams of ammonium nitrate must the outer bag contain to lower the temperature of the water from 23.0 °C...
Calculate the final temperature that will be obtained when a 10g portion of KCL is dissolved...
Calculate the final temperature that will be obtained when a 10g portion of KCL is dissolved in a coffee-cup calorimeter containing 100g of water. Specific heat of the solution is 4.084j/gc delta H sol (KCL)= 17.0kj/mol and initial temperature is 21.0. Assume that density of the solution is 1.00 g/ml and the calorimeter loses only a neglible amount of heat.
15.48 g of nickel sulfate (MM 154.75 g/mol) was dissolved in 100.00 mL of water. The...
15.48 g of nickel sulfate (MM 154.75 g/mol) was dissolved in 100.00 mL of water. The initial temperature was 20.00 oC, and the final temperature was 25.06 oC, The specific heat capacity of the reaction mixture was 4.18J/g oC. What is the temperature change T? A.20.00 oC B.25.06 oC C.22.53 oC D. 278.06K E. 5.06 oC
What is the final temperature of the solution when 4.806 g of sodium hydroxide is dissolved in 100.0 mL of water at an i...
What is the final temperature of the solution when 4.806 g of sodium hydroxide is dissolved in 100.0 mL of water at an initial temperature of 24.5 C?. The density of water is 0.9969 g/cm3, and the heat capacity is 4.184 J/C. The enthalpy of dissolution for sodium hydroxide is -44.2 kJ/mol.
Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and...
Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction: NH4NO3(s) → NH(aq) + NO3 (aq) In order to measure the enthalpy change for this reaction, 1.25 g of NH4NO3 is dissolved in enough water to make 25.0 mL of solution. The initial temperature is 25.8 °C and the final temperature (after...
Commercial cold packs consist of solid ammonium nitrate and water. NH4NO3 absorbs 330 J of heat...
Commercial cold packs consist of solid ammonium nitrate and water. NH4NO3 absorbs 330 J of heat per gram dissolved in water. In a coffee cup calorimeter, 4.00 grams of NH4NO3 is dissolved in 75.0 grams of water. Assuming that all the heat is lost from the water (specific heat = 4.81 J/gC) what is the temperature change of the water?
In a coffee cup calorimeter, 6.70 g of NH4NO3 is mixed with 75.0 g of water...
In a coffee cup calorimeter, 6.70 g of NH4NO3 is mixed with 75.0 g of water at an initial temperature of 25.0 °C. At the end of the dissolution, the final temperature of the mixture is 13.1 °C. With the assumption that the solution has the same specific heat capacity as water and is accompanied by no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in kJ/mol. en ott 46.6 94.5 47.2 3.0 80.1
Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a...
Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction: NH4NO3(s)-->NH4 ^+(aq) + NO3^-(aq). In order to measure the enthalpy change for this reaction, 1.25 g of NH4NO3 is dissolved in enough water to make 25.0 mL of solution. The initial temperature is 25.8 degrees C and the final temperature (after the...
10) (10pts) A cold pack consists of a small inner bag that contains water inside another larger bag that contains solid ammonium nitrate. When a cold pack is needed, the inner bag is broken and the water and ammonium nitrate are shaken together to dissolve the solid. If the inner bag contains 117 mL of water (density 1.00 g/mL), how many grams of ammonium nitrate must the outer bag contain to lower the temperature of the water from 23.0 °C...
Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction: NH4NO3(s) → NH(aq) + NO3 (aq) In order to measure the enthalpy change for this reaction, 1.25 g of NH4NO3 is dissolved in enough water to make 25.0 mL of solution. The initial temperature is 25.8 °C and the final temperature (after...
In a coffee cup calorimeter, 6.70 g of NH4NO3 is mixed with 75.0 g of water at an initial temperature of 25.0 °C. At the end of the dissolution, the final temperature of the mixture is 13.1 °C. With the assumption that the solution has the same specific heat capacity as water and is accompanied by no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in kJ/mol. en ott 46.6 94.5 47.2 3.0 80.1
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