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Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction:
In order to measure the enthalpy change for this reaction, 1.25g of is dissolved in enough water to make 25.0ml of solution. The initial temperature is 25.8C and the final temperature (after the solid dissolves) is 21.9C
Calculate the change in enthalpy for the reaction in kilojoules per mole. (Use 1.0g/ml as the density of the solution and 4.184 J/g*C as the specific heat capacity.)
The temperature of the solution drops by 22.4 degrees Celsius. If the specific heat of the solution is 4.18J/g degrees C, calculate the enthalpy of the solution of ammonium nitrate.
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unused lead nitrate to the container marked"sodium nitrate". What could the student do to get all the led ions out from the sodium nitrate?
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Methane has a Henry's Law constant (k) 9.88x10^-2 mol/Latm when dissolved in benzene at 25degrees C. How many grams of CH4 will dissolve in 3.00L of benzene if partial pressure is 1.48atm?
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