Calculate the heat when 100.0 ml of 0.500 m hcl is mixed with 300.0 ml of 0.590 m ba (oh) 2. assuming that the temperature of both solutions was initially 25.0Â°c and that the final mixture has a mass of 400 g and a specific heat capacity of 4.18 j/Â°c Â· g, calculate the final temperature of the mixture.

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Wells

Biology

19 November, 03:25

Calculate the heat when 100.0 ml of 0.500 m hcl is mixed with 300.0 ml of 0.590 m ba (oh) 2. assuming that the temperature of both solutions was initially 25.0Â°c and that the final mixture has a mass of 400 g and a specific heat capacity of 4.18 j/Â°c Â· g, calculate the final temperature of the mixture.

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Chaz · Answer 1

It has to be 100mL as total mass = 400g Moles HCl = 0.05; moles Ba (OH) 2 = 0.15 If volume HCl is 100mL then moles HCl = 0.05 and Ba (OH) 2 is excess If 2 moles HCl release 118 kJ then 0.05 moles HCl releases 2.95 kJ q = cm deltaT c=4.18 x 10-3 kJ/c. g DeltaT = q/cm = 2.95/4.18 x 10-3 x 400 = 1.76 degrees rise so final temp = 1.76 + 25