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An instant cold pack consists of a bag containing solid ammonium nitrate (NH, NO, and a...
2. A cold pack consists of an inner pouch containing ammonium nitrate, NHĄNO (), and an...
2. A cold pack consists of an inner pouch containing ammonium nitrate, NHĄNO (), and an outer pouch of water. Twisting the pack breaks the inner pouch and allows the water and ammonium nitrate to mix. As the ammonium nitrate dissolves, the temperature of the surroundings decreases. The energy change per mole of ammonium nitrate dissociated is 25.7 kJ. (a) Classify the reaction as endothermic or exothermic. [ans: endothermic (b) Draw a potential energy diagram for the reaction. Label the...
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...
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: NH 4 NO 3 (s)→ NH + 4 (aq)+ NO − 3 (aq) In order to measure the enthalpy change for this reaction, 1.25 g of NH 4 NO 3 is dissolved in enough water to make 25.0 mL of solution. The...
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...
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...
1. Instant cold packs used to ice athletic injuries on the field contain ammonium nitrate and...
1. Instant cold packs 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 reaction: NH4NO3 (s) à NH4 (aq) + NO3- (aq) In order to measure the enthalpy change for this reaction, 1.25 g of NH4NO3 was dissolved in 25.0 g of water. The initial temperature was 25.8 ° C and the final temperature (after all solid...
E) Mg?"(aq) + 2 NO, (aq) —> Mg(NO)>(s) 8. When solid ammonium nitrate (NH.NOs) dissolves in...
E) Mg?"(aq) + 2 NO, (aq) —> Mg(NO)>(s) 8. When solid ammonium nitrate (NH.NOs) dissolves in water, the process is endothermic, with AH solution = +25.69 kJ/mol. (This reaction has been used in commercial cold packs.) If 5,60 8 NH.NO, is dissolved in 100.0 g of water at 22.0° C, what is the final temperature of the solution? The mass of the solution is 105.6 g (100.0 8 +5,60 g = 105.68) and its specific heat capacity is 4.18 J/(8-K)....
1. A 20.0-8 piece of aluminum at 0.0°C is dropped into a beaker containing 100.0 g...
1. A 20.0-8 piece of aluminum at 0.0°C is dropped into a beaker containing 100.0 g of water. The temperature of the water drops from 90.0°C to 85.7°C. What quantity of energy did the aluminum absorb? What is the specific heat of the aluminum? 2. If 55.0 ml of water at 22.5°C is mixed with 100.0 ml of water at 95.2 'C, what would you expect for a final temperature? 3. Cold packs (the kind that get cold when you...
Experiment 13-Post-Lab Assignment 1. Athletes use cold packs containing ammonium nitrate solutions to ice their injuries....
Experiment 13-Post-Lab Assignment 1. Athletes use cold packs containing ammonium nitrate solutions to ice their injuries. A 1.25 G sample of ammonium nitrate is dissolved in 25.0 mL of water to form a solution. The temperature of the solution falls from 25.8°C to 21.9°C. Find the enthalpy of the reaction (AH ), in kJ/mol. Assume the density of water is 1.00 g/mL and the heat capacity of the total solution to be 4.184 J/g °C 2. Calculate AHⓇ in kJ/mol...
CHE201-71: General Chemistry and Quantitative Analysis I laboratory: Chapter 5 Recitation 1. When 1.025 g of...
CHE201-71: General Chemistry and Quantitative Analysis I laboratory: Chapter 5 Recitation 1. When 1.025 g of naphthalene (C16H) burns in a bomb calorimeter, the temperature rises from 24.25 °C to 32.33 "C. The heat capacity of the calorimeter is 5.86 kJ/"C. Calculate: a) Gran per mole of naphthalene for the combustion process b) gran per gram of naphthalene for the combustion process Instant cold packs, often used to ice athletic injuries on the field contain ammonium nitrate and water separated...
2. A cold pack consists of an inner pouch containing ammonium nitrate, NHĄNO (), and an outer pouch of water. Twisting the pack breaks the inner pouch and allows the water and ammonium nitrate to mix. As the ammonium nitrate dissolves, the temperature of the surroundings decreases. The energy change per mole of ammonium nitrate dissociated is 25.7 kJ. (a) Classify the reaction as endothermic or exothermic. [ans: endothermic (b) Draw a potential energy diagram for the reaction. Label 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...
E) Mg?"(aq) + 2 NO, (aq) —> Mg(NO)>(s) 8. When solid ammonium nitrate (NH.NOs) dissolves in water, the process is endothermic, with AH solution = +25.69 kJ/mol. (This reaction has been used in commercial cold packs.) If 5,60 8 NH.NO, is dissolved in 100.0 g of water at 22.0° C, what is the final temperature of the solution? The mass of the solution is 105.6 g (100.0 8 +5,60 g = 105.68) and its specific heat capacity is 4.18 J/(8-K)....
1. A 20.0-8 piece of aluminum at 0.0°C is dropped into a beaker containing 100.0 g of water. The temperature of the water drops from 90.0°C to 85.7°C. What quantity of energy did the aluminum absorb? What is the specific heat of the aluminum? 2. If 55.0 ml of water at 22.5°C is mixed with 100.0 ml of water at 95.2 'C, what would you expect for a final temperature? 3. Cold packs (the kind that get cold when you...
Experiment 13-Post-Lab Assignment 1. Athletes use cold packs containing ammonium nitrate solutions to ice their injuries. A 1.25 G sample of ammonium nitrate is dissolved in 25.0 mL of water to form a solution. The temperature of the solution falls from 25.8°C to 21.9°C. Find the enthalpy of the reaction (AH ), in kJ/mol. Assume the density of water is 1.00 g/mL and the heat capacity of the total solution to be 4.184 J/g °C 2. Calculate AHⓇ in kJ/mol...
CHE201-71: General Chemistry and Quantitative Analysis I laboratory: Chapter 5 Recitation 1. When 1.025 g of naphthalene (C16H) burns in a bomb calorimeter, the temperature rises from 24.25 °C to 32.33 "C. The heat capacity of the calorimeter is 5.86 kJ/"C. Calculate: a) Gran per mole of naphthalene for the combustion process b) gran per gram of naphthalene for the combustion process Instant cold packs, often used to ice athletic injuries on the field contain ammonium nitrate and water separated...
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