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☆☆☆☆☆No, competing side reaction is a reson why the actual yield is more than the theoretical yield.
Stoichiometry is used to find the molar ratios between the reactants of a chemical reaction.
Stoichiometry relates moles of reactant to moles of product, so if you have the amount of reactant in the equation, you can calculate the amount of product produced.
The coefficients give the ratio of moles reactant to moles product.
Models are changed if they don't fit new data.
4.2 V
The reactant that has the atom that gets oxidized
-2.37
In all areas of science
combustion and expansion
Challenges to hydrogen as fuel include no distribution network, ie gas stations, and fear that the car co u l d explode like the Hindenburg.
2Mg(s) + O2(g) ==> 2MgOMg ===> Mg^2+ + 2e- [x2 to balance electrons] = oxidation half reaction
O2 + 4e- ===> 2O^2-
So, the final oxidation half reaction will be:
2Mg(s) ===> 2Mg^2+ + 4e-
Probable "each reaction" is each reactant; coefficients are used.
