Open Question
Is the following formulation of a task correct? If not, please correct it: Complete and balance each combustion reaction equation. a. S(s) + O2(g) → b. C3H6(g) + O2(g) → c. Ca(s) + O2(g) → d. C5H12S(l) + O2(g) →
Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 103
People sometimes use sodium bicarbonate as an antacid to neutralize excess hydrochloric acid in an upset stomach. What mass of hydrochloric acid (in grams) can 2.5 g of sodium bicarbonate neutralize? (Hint: Begin by writing a balanced equation for the reaction between aqueous sodium bicarbonate and aqueous hydrochloric acid.)
Verified step by step guidance1
Write the balanced chemical equation for the reaction: \( \text{NaHCO}_3 (aq) + \text{HCl} (aq) \rightarrow \text{NaCl} (aq) + \text{H}_2\text{O} (l) + \text{CO}_2 (g) \).
Calculate the molar mass of sodium bicarbonate (NaHCO₃) using the atomic masses: Na (22.99 g/mol), H (1.01 g/mol), C (12.01 g/mol), and O (16.00 g/mol).
Determine the number of moles of sodium bicarbonate in 2.5 g by dividing the mass by its molar mass.
Use the stoichiometry of the balanced equation to find the moles of hydrochloric acid (HCl) that react with the moles of sodium bicarbonate. The mole ratio from the equation is 1:1.
Calculate the mass of hydrochloric acid by multiplying the moles of HCl by its molar mass (36.46 g/mol).
Related Practice
Textbook Question
The density of a 20.0% by mass ethylene glycol (C2H6O2) solution in water is 1.03 g/mL. Find the molarity of the solution.
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Textbook Question
Find the percent by mass of sodium chloride in a 1.35 M NaCl solution. The density of the solution is 1.05 g/mL.
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Open Question
Toilet bowl cleaners often contain hydrochloric acid, which dissolves the calcium carbonate deposits that accumulate within a toilet bowl. What mass of calcium carbonate (in grams) can be dissolved by 3.8 g of HCl? (Hint: Begin by writing a balanced equation for the reaction between hydrochloric acid and calcium carbonate.)
Textbook Question
The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)
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Textbook Question
Many home barbeques are fueled with propane gas (C3H8). What mass of carbon dioxide (in kg) is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL. (Hint: Begin by writing a balanced equation for the combustion reaction.)
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