Please Help Me?
2-How do you find qCalorimeter, qReaction, & Delta H reaction per mole of MgO consumed given the following info:
Weight of MgO= 0.705
Moles of MgO= .0175
Delta T calorimeter= 4.50 degrees C
*For this Experiment-
qCalorimeter= Ccalorimeter x Delta T calorimeter
Ccalorimeter= 418 J/degrees C=100g solution x 4.184 J/g* degrees C
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Please Help me with this. I can't figure these out. #2- was a Hess's Law experiment and I've tried plugging numbers into the formula & so many other ways but my numbers arent coming out right- they are too big. Idk what I'm doing wrong, please explain these to me! I would really appreciate it. Thanks!
Answer:
1.
y(weight) = 6.217 * x(volume)
So,
weight = 6.217 * volume
Weight/Volume = Density = 6.217 grams/mL
2.
Here, the increase in the temperature of the calorimeter is due to the heat released in the MgO reaction.
The change in heat energy of the calorimeter =
qCalorimeter= Ccalorimeter x Delta T calorimeter
qCalorimeter= 418 * 4.5 = 1881 Joules
This is the heat released by the reaction of MgO.
So qReaction = 1881 Joules
This is the heat released by 0.0175 moles of MgO. The heat released by 1 mole is called the delta H of the reaction.
So, the delta H = -1881/0.0175 = -107486 Joules = -107.486 kJ/mol.
{I have put the minus sign because the reaction is exothermic - it releases heat}
Yeah the numbers are quite big, but that doesn't mean that they are wrong.
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