Asked by Jake
2 HCl (aq) + Ba (OH2) (aq) ----> BaCl2 + 2 H20 (l)
deltaH = -118 kJ
Calculate the heat when 100.0 mL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(Oh2). Assuming that the temp. of both solutions was initially 25.0 degrees C and that the final mixture has a mass of 400.0 g and a specific capacity of 4.18 J/g degrees C, calculate the final temp of the mixture.
what's the first step to solving this problem?
deltaH = -118 kJ
Calculate the heat when 100.0 mL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(Oh2). Assuming that the temp. of both solutions was initially 25.0 degrees C and that the final mixture has a mass of 400.0 g and a specific capacity of 4.18 J/g degrees C, calculate the final temp of the mixture.
what's the first step to solving this problem?
Answers
Answered by
Charlie
i don't even understand what the problem is asking.
Answered by
DrBob222
Is that 118 kJ delta H for the reaction as written or it is per mol. I will assume it is 118 kJ as written (that is, for 2 mols HCl).
q = mass x sp.h. x (Tf - Ti)
You know q (don't forget to change to Joules), you know mass and sp.h. and Ti (initial T = 25 C). Solve for the one unknown of Tf = final T. Post your work if you get stuck.
q = mass x sp.h. x (Tf - Ti)
You know q (don't forget to change to Joules), you know mass and sp.h. and Ti (initial T = 25 C). Solve for the one unknown of Tf = final T. Post your work if you get stuck.
Answered by
Shaniqua
is it 28.53 degrees Celsius?
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