Consider the dissolution of ammonium nitrate. 1.25 g of amminum nitrate is dissolved in enough water to make 25.0 ml of solution. the initial temperature is 25.8 degc and the final temperature (after the solid dissolves) is 21.9 degc. calculate the change in enthalpy for the reaction in kj. use 1.0 g/ml as the density of solution and 4.18 j/g*degc as the specific heat capacity.

Explanation:

The expression for the calculation of the enthalpy change of a process is shown below as:-

Where,

 is the enthalpy change

m is the mass

C is the specific heat capacity

 is the temperature change

Thus, given that:-

Mass of ammonium nitrate = 1.25 g

Specific heat = 4.18 J/g°C

So,

Negative sign signifies loss of heat.

Also, 1 J = 0.001 kJ

So,

answer; i believe the correct answer is (solid gold);

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.