- #1
alexpratt
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Homework Statement
Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide
according to the equation:
2 Na(s) + 2 H2O(l) ? 2 NaOH(aq) + H2(g)
When 0.030 mol of Na is added to water, the temperature of the calorimeter rises
from 25.00C to 37.90C. If the heat capacity of the calorimeter is 400 J/C,
calculate ?H for the reaction as written
Homework Equations
q_system=-q_surroundings
q=CdeltaT
q=ndeltaH (?)
The Attempt at a Solution
i haven't actually tried to work out the numbers because I am not given the answer and i won't know if I am right or wrong. I have some ideas though which I would like someone to validate for me!
i know i can find q for the calorimeter because I am give C for the calorimeter and the temperature change. And that q of the calorimeter is -q for everything else.
So, once i have q, would i plug that into q=ndeltaH solve that for deltaH and use .03 moles for the n value?
this is the only kind of calorimetry problem i have trouble with constantly, on top of that my final exam is in two hours :( shouldn't leave things til the last minute i suppose.
anyways, any help at all is appreciated! like i said, i don't expect you to do the problem for me, i was just wondering if i could be pointed in the right direction!