How much work is done on (or by) the gases in each of the following at 298 K and 1 atm?
reaction of 5.3 g of H2(g) with 4.0 g of CO2(g) to produce H2O(g) and CO(g)
decomposition of 13.4 g KClO3 into KCl(s) and O2(g)
1) the reaction is
H2 (g) + CO2 (g)--> H2O(g) + CO (g)
We know that work = -change in number of moles X R X T
Here change in moles of reactant to product = 0
So work done = 0
2) the reaction will be
KCLO3(s) --> KCl (s) + 3/2 O2(g)
Work done =- Change in moles X R X T
Change in moles is positive so work will be done by the system
1 mole fo KClO3 will give 3/2 moles of O2
so moles of O2 produced by 13.4 grams will be
Molecular weight = 122.5 gram / mole
So moles of KCLO3 = 13.4 /22.5 = 0.109 moles
Moles of O2 produced = 0.164 moles
So work =- 0.164 X 8.314 X 298 = -408.79 Joules
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