Please help with details and steps, i am fairly loss with enthalpy and internal

Question

Please help with details and steps, i am fairly loss with enthalpy and internal energy stuff...so the more details the more i will award u with the 15000 points

In a calorimeter (e.g., a styrofoam coffee cup, which essentially prevents the flow of heat to or from the surroundings), 100.0 mL of 1.00 M NaOH and 100.0 mL of 1.00 M HCl are mixed and reacted. Both solutions were originally at 24.6 degree C. After the reaction, the final temperature of the solution is 31.3 degree C. Since the solutions are dilute, assume that all the solutions have the density and specific heat capacity of water, each rounded to two significant figures. The heat capacity of the calorimeter is insignificant. Is this reaction endothermic or exothermic? Justify your choice If heat were absorbed by this reaction in this situation, what would happen to the temperature? What is the amount of heat produced or absorbed by the reaction? Be sure to get the sign correct. What is the enthalpy change for this reaction? Express this change in units of kJ/mole H2O produced by the reaction. Be sure to get the sign correct.

Explanation / Answer

a).since tempersture is increased so heat is evolved in the surrounding

so the reaction is exothermic.

Since in acid base reaction H+ ion combines with OH- ion to form H2O

so heat will be released after formation of bond

b).The temperature would increase as can be seen from above example as well

c).Q= ms delta T

now delta T =31.3-24.6 =6.7 degree

mass of solution = (100+100)*d =200*1= 200 gm

and specific heat capacity is 4.2 J/gm

so Q= 4.2*200*6.7

= 5628 J

d).now mole is 1*0.1

= 0.1 mole

so delta H is -5628/0.1 J/mol

-56.28 KJ/mol

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