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A 24.65 apiece of iron and a 20.60 g piece of gold at 100.0 degree C...
A 28.8 g piece of iron and a 20.7 g piece of gold at 100.0°C were...
A 28.8 g piece of iron and a 20.7 g piece of gold at 100.0°C were dropped into 630.0 mL of water at 19.0°C. The molar heat capacities of iron and gold are 25.19 J/(mol·°C) and 25.41 J/(mol·°C), respectively. What is the final temperature of the water and pieces of metal?
Calculate ΔΗ for the reaction C(s)HO(g) co, given the following: - C(s) +02(g) CO(g) ΔΗ-65.85 kJ...
Calculate ΔΗ for the reaction C(s)HO(g) co, given the following: - C(s) +02(g) CO(g) ΔΗ-65.85 kJ 15 pts 5. BONUS QUESTION .+10 PTS.. directly from Smartsork Homework 3) A 23.40 g piece of iron and a 20.95 g piece of gold at 100°C were dropped into 790.0 ml. of water (density- 1.00 g/mL) at 19.50°C. The molar heat capacities of iron and gold are 25.19 J/(mol.'C) and 25.41 J/(mol.°C), respectively, and the specific heat of water is 4.184 J/(g. C)....
Exactly 10.1 mL of water at 31.0 degree C are added to a hot iron skillet....
Exactly 10.1 mL of water at 31.0 degree C are added to a hot iron skillet. All of the water is converted into steam at 100.0 degree C. The mass of the pan is 1.50 kg and the molar heat capacity of iron is 25.19 J/(mol middot degree C). What is the temperature change of the skillet? 104 degree C
A piece of metal weighing 60.922 g was heated to 100.0°C and then put into 100.0...
A piece of metal weighing 60.922 g was heated to 100.0°C and then put into 100.0 mL of water (initially at 23.7°C). The metal and water were allowed to come to equilibrium temperature, determined to be 27.8°C. A) What is the specific heat of the metal? [ Select ] B) Was the reaction endothermic or exothermic? For the water... [ Select ] For the metal... [ Select ] C) What is the identity of the metal? [ Select ] Aluminum...
Exactly 10.3 mL of water at 29.0°C is added to a hot iron skillet. All of the water is converted ...
Exactly 10.3 mL of water at 29.0°C is added to a hot iron skillet. All of the water is converted into steam at 100.0°C. The mass of the pan is 1.30 kg and the molar heat capacity of iron is 25.19 J/mol C). What is the temperature change of the skillet? oC
Exactly 10.3 mL of water at 29.0°C is added to a hot iron skillet. All of the water is converted into steam at 100.0°C. The mass of the...
Exactly 10.3 mL of water at 31.0 degree C are added to a hot iron skillet....
Exactly 10.3 mL of water at 31.0 degree C are added to a hot iron skillet. All of the water is converted into steam at 100 degree C. The mass of the pan is 1.15 kg and the molar heat capacity of iron is 25.19 J/(mol middot degree C). What is the temperature change of the skillet? The temperature of the skillet goes down, not up. Remember, the heat gained by the water is LOST by the skillet: Q_skillet =...
Exactly 17.8 mL of water at 28.0 °C is added to a hot iron skillet. All...
Exactly 17.8 mL of water at 28.0 °C is added to a hot iron skillet. All of the water is converted into steam at 100.0°C. The mass of the pan is 1.45 kg and the molar heat capacity of iron is 25.19 J/(mol·°C). What is the temperature change of the skillet?
5) If 78.6 g piece of iron is dropped into 100.0 g of water initially at 24.6 °C. The final temperature of both wat...
5) If 78.6 g piece of iron is dropped into 100.0 g of water initially at 24.6 °C. The final temperature of both water and iron was measure at 28.5 °C. Calculate the initial temperature of iron? (Specific heat of water and iron from #1)
please help me. Thanks A piece of copper metal weighing 36.3 g is initially at 100.0...
please help me. Thanks
A piece of copper metal weighing 36.3 g is initially at 100.0 degree C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0 degree C. After stirring, the final temperature of both copper and water is 25.0 degree C. Assuming no heat losses, an that the specific heat capacity of water is 4.184 J/g degreeC, what is the specific heat capacity of the copper in J/g degreeC?
A 29.3 g piece of metal is heated to 97 degree C and dropped into a...
A 29.3 g piece of metal is heated to 97 degree C and dropped into a calorimeter containing 50.0 g of water (specific heat capacity of water is 4.18 J/g degree C) initially at 22.9 degree C. The empty calorimeter has a heat capacity of 125 J/K. the final temperature of the water is 25.96 degree C. Ignoring significant figures., calculate the specific heat of the metal. A) 0.481 J/gK. B) 0.361 J/gK C) 0.120 J/gK D) 0.300 J/gK E)...
Calculate ΔΗ for the reaction C(s)HO(g) co, given the following: - C(s) +02(g) CO(g) ΔΗ-65.85 kJ 15 pts 5. BONUS QUESTION .+10 PTS.. directly from Smartsork Homework 3) A 23.40 g piece of iron and a 20.95 g piece of gold at 100°C were dropped into 790.0 ml. of water (density- 1.00 g/mL) at 19.50°C. The molar heat capacities of iron and gold are 25.19 J/(mol.'C) and 25.41 J/(mol.°C), respectively, and the specific heat of water is 4.184 J/(g. C)....
Exactly 10.1 mL of water at 31.0 degree C are added to a hot iron skillet. All of the water is converted into steam at 100.0 degree C. The mass of the pan is 1.50 kg and the molar heat capacity of iron is 25.19 J/(mol middot degree C). What is the temperature change of the skillet? 104 degree C
Exactly 10.3 mL of water at 29.0°C is added to a hot iron skillet. All of the water is converted into steam at 100.0°C. The mass of the pan is 1.30 kg and the molar heat capacity of iron is 25.19 J/mol C). What is the temperature change of the skillet? oC
Exactly 10.3 mL of water at 29.0°C is added to a hot iron skillet. All of the water is converted into steam at 100.0°C. The mass of the...
Exactly 10.3 mL of water at 31.0 degree C are added to a hot iron skillet. All of the water is converted into steam at 100 degree C. The mass of the pan is 1.15 kg and the molar heat capacity of iron is 25.19 J/(mol middot degree C). What is the temperature change of the skillet? The temperature of the skillet goes down, not up. Remember, the heat gained by the water is LOST by the skillet: Q_skillet =...
5) If 78.6 g piece of iron is dropped into 100.0 g of water initially at 24.6 °C. The final temperature of both water and iron was measure at 28.5 °C. Calculate the initial temperature of iron? (Specific heat of water and iron from #1)
please help me. Thanks
A piece of copper metal weighing 36.3 g is initially at 100.0 degree C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0 degree C. After stirring, the final temperature of both copper and water is 25.0 degree C. Assuming no heat losses, an that the specific heat capacity of water is 4.184 J/g degreeC, what is the specific heat capacity of the copper in J/g degreeC?
A 29.3 g piece of metal is heated to 97 degree C and dropped into a calorimeter containing 50.0 g of water (specific heat capacity of water is 4.18 J/g degree C) initially at 22.9 degree C. The empty calorimeter has a heat capacity of 125 J/K. the final temperature of the water is 25.96 degree C. Ignoring significant figures., calculate the specific heat of the metal. A) 0.481 J/gK. B) 0.361 J/gK C) 0.120 J/gK D) 0.300 J/gK E)...
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