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![Q5 -Heat lost by metals Heat gain by water iongolwa volume of water-790.0ml, Density of water= 1.00g/ml so, mass of water-790.0g Moles of iron 23.40g*1 mole /55.85g 0.419 moles Moles of gold-20.95g*1 mole / 196.97g = 0.106 moles -[0.419 moles* 25.19/mole.oCYTf-100) oC]-[ 0.106 moles * 25.41/mole.oC* (Tf-100)C-790.0g* 4.184J /g°C* (Tf-19.15)°C -[10.55 *(Tf-100) °C] 12.69 * (Tf-100)°C] 3305.36 *(Tf-19.15)°C [10.55 Tf-1055] [2.69Tf -269] 3305.36Tf -64454.52 10.55 Tf +1055] -2.69Tf +269 3305.36Tf -64454.52 1055 +269 +64454.52 3305.36Tf +10.55Tf +2.69Tf 65778.52 = 3318·6Tf Tf = 19.82°C Final temperature ofwater and pieces of metal = 19.82°C](http://img.homeworklib.com/questions/ee277f80-4ef6-11eb-9998-854f3d804d85.png?x-oss-process=image/resize,w_560)
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Calculate ΔΗ for the reaction C(s)HO(g) co, given the following: - C(s) +02(g) CO(g) ΔΗ-65.85 kJ...
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?
A 24.65 apiece of iron and a 20.60 g piece of gold at 100.0 degree C...
A 24.65 apiece of iron and a 20.60 g piece of gold at 100.0 degree C were dropped into 770.0 mL of water at 21.70 degree C. The molar heat capacities of iron and gold are 25.19 J/(mol degree C) and 25.41 J/(mol, degree C), respectively. What is the final temperature of the water and pieces of metal?
3) If 28.0 g of water at 26.4 °C gain 5,563 J of heat, what is...
3) If 28.0 g of water at 26.4 °C gain 5,563 J of heat, what is the final temperature of water? (Specific heat of water is 4.184 J/g.°C)) 4) If 46.2 g piece of aluminum is cooled from 84.5 °C to 29.5 °C, how much energy was lost by aluminum? (specific heat of aluminum is 0.901 J/(g.°C)) 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...
15.2 J of heat is applied to 8.0 g samples of each of the following substances:...
15.2 J of heat is applied to 8.0 g samples of each of the following substances: water (s), water (g), mercury (1), and gold (s). Which substance's temperature will increase the most? The Specific Heat Capacities of Some Common Substances Substance Specific Heat Capacity (J/g °C) water (()* (liquid) 4.184 water(s) (ice) 2.03 water (8) (steam) 2.0 aluminum (s) 0.89 iron (s) 0.45 mercury (1) 0.14 0.71 silver (S) 0.24 gold (s) 0.13 *The symbols (s), (), and (g) indicate...
4. Heat transfer: q = mass x Cs x ΔT and –qreaction = +qsolution a. A...
4. Heat transfer: q = mass x Cs x ΔT and –qreaction = +qsolution a. A piece of metal with a mass of 8.6 g was heated to 100.0°C and dropped into a coffee cup calorimeter containing 402.4 g of water at 25.0°C. If the temperature of the water and the metal at thermal equilibrium is 26.4°C, what is the specific heat of this metal in J/g°C? b. How much heat energy must be added in order to boil a...
Calorimetry 1. Consider the following data: 4.99 g g 50 g 24 C 38.7 °C 111.1...
Calorimetry 1. Consider the following data: 4.99 g g 50 g 24 C 38.7 °C 111.1 g/mol Mass of CaCl Mass of Water Intial Temperature Final Temeprature Molar Mass of CaCl2 (a) Calculate the heat of solution. (AH) Assume that the specific heat of the solution is the same as water, 4.184 J/g- C and that no heat is gained or lost by the cup. (4 pts) (b) Calculate the number of moles of CaCl2. (3 pts) (c) Calculate the...
QUESTION 19 A 63.1 g piece of metal whose T - 73.8 °C is placed in...
QUESTION 19 A 63.1 g piece of metal whose T - 73.8 °C is placed in a coffee cup calorimeter containing 155 g water. When the system reaches equilibrium, the water has changed from 19.20 °C to 23.40°C. What is specific heat of metal? Density of water is 1.00 g/ml. Specific heat of H 20 is 4.184/gºo. 0.483 J/g °C 0.900 J/g °C 3.82 J/g °C 0.0150J/g °C 0.237 J/g °C 0.856 J/g °C 3.53 J/g °C 0.981 J/g °C
Calculate the in kJ/mole given that the following reaction has a = -1219.26 kJ/mol 2 ClF3(g)...
Calculate the in kJ/mole given that the following reaction has a = -1219.26 kJ/mol 2 ClF3(g) + 2 NH3(g) ----- > N2(g) + 6 HF(g) + Cl2(g) Use data in appendix III (b) The military uses FRH’s (Flameless ration heaters) to heat MRE’s (meals ready to eat). (Heat of formation of Mg( OH)2(Aqua) = -926.8 kJ/mole One of the reactions used in an FRH is Mg(s) + 2 H2O(l) ------ > Mg(OH)2(aq) + H2(g) Using data in Appendix III...
A 296.0 g piece of granite, heated to 601.0°C in a campfire, is dropped into 1.10...
A 296.0 g piece of granite, heated to 601.0°C in a campfire, is dropped into 1.10 L water (d = 1.00 g/mL) at 25.0°C. The molar heat capacity of water is cp,water = 75.3 J/(mol ·°C), and the specific heat of granite is cs,granite = 0.790 J/(g ·°C). Calculate the final temperature of the granite.
A 301.0 g piece of granite, heated to 561.0°C in a campfire, is dropped into 1.00...
A 301.0 g piece of granite, heated to 561.0°C in a campfire, is dropped into 1.00 L water (d = 1.00 g/mL) at 25.0°C. The molar heat capacity of water is cp,water = 75.3 J/(mol ·°C), and the specific heat of granite is cs,granite = 0.790 J/(g ·°C). Calculate the final temperature of the granite.
A 24.65 apiece of iron and a 20.60 g piece of gold at 100.0 degree C were dropped into 770.0 mL of water at 21.70 degree C. The molar heat capacities of iron and gold are 25.19 J/(mol degree C) and 25.41 J/(mol, degree C), respectively. What is the final temperature of the water and pieces of metal?
3) If 28.0 g of water at 26.4 °C gain 5,563 J of heat, what is the final temperature of water? (Specific heat of water is 4.184 J/g.°C)) 4) If 46.2 g piece of aluminum is cooled from 84.5 °C to 29.5 °C, how much energy was lost by aluminum? (specific heat of aluminum is 0.901 J/(g.°C)) 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...
15.2 J of heat is applied to 8.0 g samples of each of the following substances: water (s), water (g), mercury (1), and gold (s). Which substance's temperature will increase the most? The Specific Heat Capacities of Some Common Substances Substance Specific Heat Capacity (J/g °C) water (()* (liquid) 4.184 water(s) (ice) 2.03 water (8) (steam) 2.0 aluminum (s) 0.89 iron (s) 0.45 mercury (1) 0.14 0.71 silver (S) 0.24 gold (s) 0.13 *The symbols (s), (), and (g) indicate...
Calorimetry 1. Consider the following data: 4.99 g g 50 g 24 C 38.7 °C 111.1 g/mol Mass of CaCl Mass of Water Intial Temperature Final Temeprature Molar Mass of CaCl2 (a) Calculate the heat of solution. (AH) Assume that the specific heat of the solution is the same as water, 4.184 J/g- C and that no heat is gained or lost by the cup. (4 pts) (b) Calculate the number of moles of CaCl2. (3 pts) (c) Calculate the...
QUESTION 19 A 63.1 g piece of metal whose T - 73.8 °C is placed in a coffee cup calorimeter containing 155 g water. When the system reaches equilibrium, the water has changed from 19.20 °C to 23.40°C. What is specific heat of metal? Density of water is 1.00 g/ml. Specific heat of H 20 is 4.184/gºo. 0.483 J/g °C 0.900 J/g °C 3.82 J/g °C 0.0150J/g °C 0.237 J/g °C 0.856 J/g °C 3.53 J/g °C 0.981 J/g °C
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