Answer:
69.55 (w/w) %
Explanation:
When NaHCO3 reacts with an acid HA, the reaction that occurs is:
NaHCO3 + HA → H2O + NaA + CO2
<em>Where 1 mole of NaHCO3 produce 1 mole of CO2</em>
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Thus, we need to convert the mass of CO2 to moles using its molar mass (44g/mol). Then, based on the chemical equation, moles of CO2 produced are equal to moles of NaHCO3 in the mixture. With its molar mass -84g/mol- we can find the mass of NaHCO3 and mass percent:
<em>Moles CO2:</em>
0.561g * (1mol / 44g) = 0.01275 moles CO2 = Moles NaHCO3.
<em>Mass NaHCO3:</em>
0.01275 moles * (84g/mol) = 1.071g NaHCO3
<em>Mass percent:</em>
1.071g NaHCO3 / 1.54g sample * 100
<h3>69.55 (w/w) %</h3>
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Answer:
0.500 mole of Xe (g) occupies 11.2 L at STP.
General Formulas and Concepts:
<u>Gas Laws</u>
- STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 K
<u>Stoichiometry</u>
- Mole ratio
- Dimensional Analysis
Explanation:
<u>Step 1: Define</u>
<em>Identify.</em>
0.500 mole Xe (g)
<u>Step 2: Convert</u>
- [DA] Set up:

- [DA] Evaluate:

Topic: AP Chemistry
Unit: Stoichiometry
Answer:
5.0 38 84.0 749.7 528.0 729.0 738.9 739.0