Chemical Reactions: Physical Chemistry
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1. Some sulfuric acid is spilled on a lab bench. It can be neutralized by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid as follows.
2 NaHCO3(s) + H2SO4(aq) Na2SO4(aq) + 2 H2O(l) + 2 CO2(g)
Sodium bicarbonate is added until the fizzing due to the formation of CO2(g) stops. If 26 mL of 6.0 M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid? (g)
2. Nitrogen and oxygen gases react to form dinitrogen trioxide gas.
2 N2(g) + 3 O2(g) 2 N2O3(g)
At a certain temperature and pressure 4.2 L of N2 reacts with 6.3 L of O2. If all the N2 and O2 are consumed, what volume of N2O3, at the same temperature and pressure, will be produced? (L)
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1.
Some sulfuric acid is spilled on a lab bench. It can be neutralized by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid as follows.
2NaHCO3(s) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) + 2CO2(g)
Sodium bicarbonate is added until the fizzing due to the formation of CO2(g) stops. If 26 mL of 6.0M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid? (g)
To completely neutralize the acid we see that for every mole of acid we need two moles of Sodium Bicarbonate (the ...
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