🤓 Based on our data, we think this question is relevant for Professor Blankenship's class at UGA.
Notice that we are given the mass of both reactants: this means we need to determine the limiting reactant, which is the reactant that forms the less amount of product.
This is because once the limiting reactant is all used up, the reaction can no longer proceed and make more products.
This means the limiting reactant determines the maximum mass of the product (CO2) formed.
We need to perform a mole-to-mole comparison between each reactant and CO2.
Balanced Reaction: NaHCO3(s) + HCl(aq) → NaCl(aq) + H2O(l) + CO2(g)
For NaHCO3: From the balanced equation, 1 mole of NaHCO3 form 1 mole of CO2.
The moles of CO2 formed by 8.67 g NaHCO3 is:
Sodium bicarbonate reacts with hydrochloric acid in a gas-forming reaction to produce aqueous sodium chloride, water, and carbon dioxide gas:
NaHCO3(s) + HCl(aq) → NaCl(aq) + H2O(l) + CO2(g)
Determine the mass of CO2 gas produced when 8.67 g of NaHCO3 is added to a solution that contains 5.65 g of HCl.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Blankenship's class at UGA.