Question

1. A student accidentally spills a 1.00 L bottle of concentrated 18.0 M sulfuric acid (silly student) on the floor of the laboratory. She attempts to neutralize the spill by pouring a 5.0 kg box of baking soda (sodium hydrogen carbonate) onto the acid. a. Write a balanced NET IONIC equation for the reaction. $2H^+ + 2HCO_3^- \rightarrow 2H_2O + 2CO_2$ b. What is the limiting reagent? c. How many grams of sodium hydrogen carbonate are required to neutralize the acid? d. How many moles of excess reactant remain after all the limiting reactant has been consumed? e. Would a floor consisting of bare concrete require more, less or the same amount of baking soda to neutralize the spill? Explain.

          1. A student accidentally spills a 1.00 L bottle of concentrated 18.0 M sulfuric acid (silly student) on the floor of the laboratory. She attempts to neutralize the spill by pouring a 5.0 kg box of baking soda (sodium hydrogen carbonate) onto the acid.
a. Write a balanced NET IONIC equation for the reaction.
$2H^+ + 2HCO_3^- \rightarrow 2H_2O + 2CO_2$
b. What is the limiting reagent?
c. How many grams of sodium hydrogen carbonate are required to neutralize the acid?
d. How many moles of excess reactant remain after all the limiting reactant has been consumed?
e. Would a floor consisting of bare concrete require more, less or the same amount of baking soda to neutralize the spill? Explain.

1 a student accidentally spills a 100 l bottle of concentrated 180 m sulfuric acid silly student on the floor of the laboratory she attempts to neutralize the spill by pouring a 50 kg box of 25675

Added by Fernando G.

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