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Question 10 3 pts A 126 gram sample of ice was heated from -11.4°C to 42°C....
3 pts Question 11 A 126 gram sample of ice was heated from 11.4°C to 42°C. The Specific Heat of ice = 2.09 J/gºC; Specific Heat of water = 4.184 J/gºC; and the Heat of fusion of ice = 334 J/g. Calculate the heat required to form liquid H2O up to 42°C. 221x104) 1.11 x 104) -2.21 x 104) -1.11 x 104)
ockhart 3 pts Question 12 A 126 gram sample of ice was heated from -11.4°C to 42°C. The Specific Heat of ice = 2.09 J/gºC; Specific Heat of water = 4.184 J/gºC; and the Heat of fusion of ice = 334 J/g. Calculate the total amount of heat required to convert 126 grams of ice at -11.4°C to water at 42°C. 2.51x 104) 4.60 x 104) 1.41x 104 6.72 x 104
15. A coffee cup calorimeter contains 400.0 g of water and 25.0 g of ice at 0.0 °C. When a 35.00 g scoop of calcium chloride (also at 0.0 °C) is added to the ice water, the calcium chloride dis- solves as shown. The heat produced by this reaction is enough to melt all of the ice and warm up the resulting calcium chloride solution. What is the final temperature of this solution? Assume there is no heat lost to...
A 57.09 gram sample of iron (with a heat capacity of 0.450 J/gºC) is heated to 100.0 ºC. It is then transferred to a coffee cup calorimeter containing 45.11 g of water (specific heat of 4.184 J/ gºC) initially at 20.63 ºC. If the final temperature of the system is 23.59ºC, how much heat was absorbed by the calorimeter? (Please give the absolute value) J
An ice cube with a mass of 46.4 g at 0.0 ∘C is added to a glass containing 4.20×102 g of water at 45.0 ∘C . Determine the final temperature of the system at equilibrium. The specific heat capacity of water, ?s , is 4.184 J/g⋅∘C , and the standard enthalpy of fusion, Δ?∘fus , of water is 6.01×103 J/mol . Assume that no energy is transferred to or from the surroundings.
An ice cube with a mass of 53.0 g at 0.0 °C is added to a glass containing 368 g of water at 45.0 °C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, Cs, is 4.184 J/g·°C and the standard enthalpy of fusion, ΔH°fus, of water is 6.01 × 103 J/mol. Assume that no energy is transferred to or from the surroundings.
Ice at -42 C was warmed to steam at 134 C. How much energy, in calories, was gained to warm 250 g of ice to steam? (get the sign right!) Specific heat H2O(g) = 0.48 cal/gram-C, Specific heat H2O(s) = 0.5 cal/gram-C. Specific heat H2O(l) = 1.0 cal/gram-C. Heat of vaporization H2O = 540 cal/gram, Heat of fusion H2O = 80 cal/gram.
Please help 1. Calculate the increase of entropy (in J/K) when 42 g of ice melts at 0 ºC and 1 atm. (The heat of fusion for ice is 6,000 J/mol.) 2. Calculate the change in entropy (in J/K) when a 34.0 g of water is heated from 12.4 ºC to 70.5 ºC at 1 atm. (The specific heat is 4.184 J/(g-K).) Notice that entropy and heat capacity have the same units.
A 61.93 gram sample of iron (with a specific heat of 0.450 J/g °C) is heated to 100.0 °C. It is then transferred to a coffee cup calorimeter containing 40.6 g of water (specific heat of 4.184 J/ g °C) initally at 20.63 °C. If the final temperature of the system is 23.59, what was the heat absorbed (q) of the calorimeter? (total heat absorbed by the water and calorimeter = heat released by the iron)
What is the final temperature, (in oC), after a 26.5 gram piece of ice at 0oC is placed into a styrofoam cup with 117.0 grams of water initially at 76.5oC? Assume no loss or gain of heat from the surroundings. Enter your answer without units. heat of fusion of water is 333 J/g. The specific heat of H2O(l) is approximately constant at 4.184 J/gK.