Based on the thermodynamic properties provided for water, determine the amount of energy released for 155.0 g of water to go from 39.0 °c to -36.5°c. property melting point boiling point ahfus ahvap cp (s) value 0.0 100.0 6.01 40.67 37.1 75.3 33.6 units oc kj/mol kj/mol j/mol. oc j/mol c mol oc cp (g)

Answer : The amount of energy released will be, -88.39 kJ

Solution :

The process involved in this problem are :

The expression used will be:

where,

= heat available for the reaction = ?

m = mass of water = 155.0 g

= specific heat of solid water =

= specific heat of liquid water =

= enthalpy change for fusion =

Molar mass of water = 18 g/mole

Now put all the given values in the above expression, we get:

Therefore, the amount of energy released will be, -88.39 kJ

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

what is the question here. i think you messed up.