What is the mass of ice (in g) at 0 °C that can be completely melted into liquid water at 0°C by a 119 g aluminum block at temperature 112 °C? Assume the aluminum block can melt the ice until its temperature drops to 0 °C. The heat capacity of aluminum is 0.903 J g-1 °C-1 and the heat of fusion of water is 6.02 kJ mol-1. Express your answer to 3 significant figures.
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What is the mass of ice (in g) at 0 °C that can be completely melted...
How much ice (in grams) should be melted to lower the temperature of 350 mL of water from 25 ∘C to 5 ∘C ? (Assume the following: the density of water is 1.0 g/mL, the ice is at 0 ∘C, and the heat of fusion of ice is 6.02 kJ/mol.) Express your answer using two significant figures.
How much ice (in grams) should be melted to lower the temperature of 350 mL of water from 25 ∘C to 5 ∘C ? (Assume the following: the density of water is 1.0 g/mL, the ice is at 0 ∘C, and the heat of fusion of ice is 6.02 kJ/mol.) Express your answer using two significant figures
An ice cube of mass 8.5 g at temperature 0∘C is added to a cup of coffee, whose temperature is 90 ∘C and which contains 130 g of liquid. Assume the specific heat capacity of the coffee is the same as that of water. The heat of fusion of ice (the heat associated with ice melting) is 6.0 kJ/mol. Find the temperature of the coffee after the ice melts.(in C)
You have a block of ice at a temperature of -100°C. This block of ice is made from 180g H2O. The block of ice will be heated continually until it becomes super-heated steam at a temperature of 200°C Cice = 2.03 J/g-K ΔHfus=6.01 kJ/mol Cwater = 4.18 J/g-K Csteam = 1.84 J/g-K ΔHvap=40.67 kJ/mol What is the enthalpy change raising the temperature of 180 g of ice at −100 °C to 0°C? What is the enthalpy change upon melting 180...
Initial mass of ice = 150.89 g Final mass of ice = 99.69 g Initial temperature of water = 42 °C Final temperature of water = 0.4 °C Determine the mass of the ice that has melted. Determine the variation of the water temperature (ΔT). a) Calculate the energy (in J) released by 100 g of water when it cooled by ΔT. The specific heat capacity(c) of water is 4.18 J/(g°C). Use the formula Q = mcΔT and the mass...
ch.11 Four ice cubes at exactly 0 ºC with a total mass of 52.0 g are combined with 135 g of water at 90 °C in an insulated container. (AH..-6.02 kJ/mol. Cwater-4.18J/ 6C) V Part A If no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer using two significant figures. OVO AXT ? Given that the heat of freezing of water is-6.02 kJ/mol, that the heat capacity of H.O() is 752...
Calculate how many grams of ice at 0°C would be melted by 100 g of 100°C steam. Hint: heat will be transferred from the steam to the ice in two processes: •the steam will condense into liquid, and •that liquid will transfer heat until it is at the freezing point of water. Note that for water: Lf = 80 cal/g (ice), and Lv = 540 cal/g (steam) (Use calories) C(water) =1 cal/g*C Answer in grams no decimal places.
How much heat required to convert 36 grams (2 moles) of ice at 0 degrees C to liquid water at 50 degrees C? delta-H of fusion for H2O is 6.02 kJ/mol and the heat capacity of liquid water is 4.18J/g degrees C. A) 12 kJ B) 7524 J C) 8728 J D) 19564 J
A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0 g of liquid water at 60 degrees C. a) Sketch the heating curve on the axis for the melting of 75g of ice at 0 degrees C followed by the subsequent heating of the water formed to 60 degrees C. b) What is the total heat needed to melt the 75g of ice? c) What is the total amount of heat required to raise the...
1. 0.25-mol ice at -5 °C is mixed with n-mol hot water initially at 45 °C in an isobaric adiabatic calorimeter at 1 atm. The final temperature of the mixture becomes 10 °C, and the ice is melted into liquid water. Assume the density of ice is 0.917 g/mL and the density of water is 1.000 g/mL. The molar heat capacity Com of liquid water is 75.291 J/mol K, the molar heat capacity Cm of ice is 38.09 J/mol-K, and...