In Lab 8 you will be determining the enthalpy change accompanying various phase

Question

In Lab 8 you will be determining the enthalpy change accompanying various phase changes. In this pre-lab assignment you will go through some of the calculations required for Part 2 of this experiment, in which you determine Delta H fusion of ice. To determine Delta H fusion of ice you will essentially add ice to water, allow the ice to melt, and note the temperature change of the water. Let's first get an idea of the ratio of water to ice that you will need. The value for the Delta H fusion of ice is 6.0 kJ/mol. Let's suppose you start with 39.9 g of ice. Determine Delta H for melting 39.9 g of ice. 13300 J Previous Tries Now let's suppose you add the 39.9 g of ice to water at a normal temperature in the lab (25degreeC). If you want to add the ice to a minimum amount of water to melt all of the ice, what will be the final temperature of the water in the calorimeter after all of the ice has melted? 0degreeC Previous Tries What is the minimum mass of 25degreeC water required to melt all 39.9 g of ice? g Tries 2/99 Previous Tries

Explanation / Answer

For water:
Qwater=Q=MCp?T
M=mas
Cp=4.2
?T= 25+273- (0+273)= 25 K
Q= M(4.2)(25)= 105*M .KJ/kg


For ice
Q= Latent heat(Mass)
= 336J/g( 39.9)
= 13406.4 J=13.406KJ

therefore:
420M= 13.406
M= 13.406KJ/ 105 KJ/kg
= 0.1276 kg
= 127.6 g.

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