[References) A 18.0-g sample of ice at -13.6°C is mixed with 105.1 g of water at 80.0°C. Calculate the final temperatur...
A 18.7-g sample of ice at -13.1°C is mixed with 118.5 g of water at 80.0°C. Calculate the final temperature of the mixture, assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.03 and 4.18 J/g∙°C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol.
ا ما حال ده اند A 13.6-g sample of ice at -14.8°C is mixed with 101.5 g of water at 80.0°C. Calculate the final temperature of the mixture, assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(1) are 2.03 and 4.18 J/g.°C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol. Final temperature = °C
step by step solution please A 24.0-g sample of ice at –12.1°C is mixed with 104.2 g of water at 80.0°C. Calculate the final temperature of the mixture, assuming no heat loss to the surroundings. The heat capacities of and are 2.03 J/g⋅°C and 4.18 J/g⋅°C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol. Temperature = ? °C
Calculate the heat required in Joules to convert 18.0 grams of water ice at a temperature of -20° C to liquid water at the normal boiling point of water. Given: -specific heat of ice = 2.09 J/g°C -specific heat of liquid water = 4.184 J/g°C -specific heat of water vapor = 2.03 J/g°C -molar heat of fusion of water = 6.02 kJ/mol -molar heat of vaporization of water = 40.7 kJ/mol
9. Four ice cubes exactly at-50 °C with a total mass of 53.5 g are combined with 1 15 g of water at 75 °C in an insulated container. If no heat is lost to the surroundings, what is the final temperature of the mixture? The heat capacity of ice is 2.03 JIg C and that of water is 4.18 JIg C. The heat of fusion of water is +6.01 kJ/mol. (1.5 pts) 9. Four ice cubes exactly at-50 °C...
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 24.1 g of steam at 158°C is condensed, cooled, and frozen to ice at -50.°C.
References Calculate the change in entropy that occurs when 18.02 g of ice at -12.5C is placed in 45,04 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 JK-mol-and 753 JK mol", respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy - JK Submit Answer T ry Another Version 3tem attempts remaining
How much heat (in kJ) is needed to convert an 18.0-g cube of ice at 0.0 oC into liquid water at 20.0 oC? For water (H2O): heat of fusion = 6.02 kJ/mol, specific heat capacity (liquid) = 4.18 J/g oC. a) 1.61 kJ b) 7.52 kJ c) 89.6 kJ d) 518 kJ
2. 44.0 g of ice at –20.0 °C is mixed with 325 g of water at 32.1 °C. Calculate the final temperature of the mixture. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/g-K, liquid water = 4.184 J/g-K) ***HINT: Remember that ice melts at 0 °C***
6) There is 15.0 g of ice at 0.0C. How many grams of water at 50.0C must be added to the ice to melt all the ice and keep the temperature of the mixture at 0.OC? H2O(s)= 2.06J/gc Specific heat: H2O(0) = (4.18 J/g C) H20 heat of vaporization=2260 J/g H2O(g)=(2.03 J/g C) H2O heat of fusion=333 J/g b)25 8 c)23.98 d)7. 58 )0.428