Focus Questions: What is the heat of neutralization for a strong acid/strong bas
ID: 958041 • Letter: F
Question
Focus Questions: What is the heat of neutralization for a strong acid/strong base reaction? 2. What is the identity of your unknown metal? 3. What is the molar heat of solution of ammonium chloride salt? 2. The reaction done in this lab was exothermic. Do you think it would be possible to use a coffee cup and a thermometer to measure the AH value of an endothermic reaction? Explain. 3. Write the net ionic equation for the reaction between hydrochloric acid and aqueous sodium hydroxide reaction. How would the temperature change and the calculated heat of neutralization vary if the concentration of the acid and the base used in this experiment will double? Explain. 4. In a coffee-cup calorimeter, 1.80 g of NH4NO3 is mixed with 74.0 g of water at an initial temperature of 25.00 degree C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.07 degree C. Assuming the solution has a heat capacity of 4.18)/degree C-g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kj/mol.Explanation / Answer
2. Is it possible to measure the enthalpy change of an endothermic reaction usin a cup of coffe and thermometer.
Yes, it is possible. We can treat the coffee as water based on the fact is mostly water, so the Cp would be the same of the water, Cp=4,18KJ/Kg*°C.
If we put a glass with the endothermic reaction solution in the cup with coffee, most of the heat needed in the reaction would be extracted from the coffee. so calculating the enthalpy change of the coffee we will know the reaction entalpy.
The formula to calculate the coffee entalpy change is
DeltaH=m*Cp*(T2-T1)
m= mass of coffee/water
Cp=calorific constant of coffee/water
T2-T1= temperture change measured with the thermometer
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