A metal with a molar mass of 192.22 g mol-1 and an atomic radius of 1.80 x 102 pm packs in a face...
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...
A solution containing 2.610 g of CuSO_4.5H_2O (molar mass 249.7 g mol^-1) is completely reacted with excess Zn metal in a constant pressure calorimeter, according to: Cu^2 + + Zn rightarrow Cu + Zn^2 + (a) Determine delta H for the reaction as written above if a temperature change of 4.319 K is measured in the reaction mixture. Assume that the combined heat capacity of the calorimeter and solution is 526.37 J K^-1. (b) Is the enthalpy change determined in...
The constant-pressure molar heat capacity of H2O (s) and H2O (l) is 75.291 J K−1 mol−1 and that of H2O (g) is 33.58 J K−1 mol−1 . Assume that the constant-pressure molar heat capacities are constant over the studied temperature range. Calculate the change in entropy of the system when 15.0 g of ice at −12.0 °C is converted to water vapour at 105.0 °C at a constant pressure of 1 bar!
An unknown compound has a molar mass of 245 g/mol and an enthalpy of solvation of 13 kJ/mol. What is the final temperature of 273 mL of water with an initial temperature of 55 °C, if a student completely dissolves 19 grams of the unknown compound? (heat capacity of water = 4.18 J/g °C)
Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T, of the water after all the ice melts. heat capacity of H2O(s) heat capacity of H2O(1) enthalpy of fusion of H,O 37.7 J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti =
The change in enthalpy when 1 mol of ice is melted at 273K is 6008 J Heat Capacity of liquid water, Cp_{L} = 75.44 J/mol K Heat Capacity of solid water, Cp_{S} = 38J/mol K Enthalpy chage of melting at 273K, \Delta H_{273}=6008 J Calculate the standard enthalpy of fusion for ice. Calculate the heat released when 100 g of water supercooled at 250K solidify Initial T=25°C=298K Thanks
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...
Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T. of the water after all the ice melts. heat capacity of H,O() heat capacity of H,O(1) enthalpy of fusion of H,0 37.7J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti = 24.99 "C Incorrect
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.
1) Aluminum has a density of 2.699 g/cm3, and the radius of the aluminum atom is 143 pm. Verify that the metal crystallizes as a face-centered cube. EX. 3 Calculate the percentage of the total volume is occupied by spheres in (a) a simple cube, (b) a body-centered cube, and (c) a face-centered cube in which all atoms are identical. (b) A body-centered cube (bcc)