{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

BalloonRaceLRDemo - The Great Balloon Race Background We...

Info iconThis preview shows pages 1–4. Sign up to view the full content.

View Full Document Right Arrow Icon
The Great Balloon Race Background: We will be reacting various amounts of sodium bicarbonate with a constant amount of acetic acid (see table 1) resulting in the following reaction: NaHCO 3 (s) + CH 3 COOH (aq) barb2right NaCH 3 CO 2 (aq) + CO 2 (g) + H 2 O (l) The resulting CO 2 (g) produced will cause the balloons to inflate. Table 1: Flask Number: Amount of NaHCO 3 (s) Amount of CH 3 CO 2 H (aq) 1 0.50 g 0.030 moles 2 1.50 g 0.030 moles 3 3.00 g 0.030 moles Pre Race Questions: 1. Which balloon do you believe will inflate the fastest? Why? 2. Which balloon do you believe will inflate the most? Why?
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
NaHCO 3 (s) + CH 3 COOH (aq) barb2right NaCH 3 CO 2 (aq) + CO 2 (g) + H 2 O (l) Post Race Questions: 3. Which balloon inflated the fastest? Why? 4. Which balloon inflated the most? Why? 5. Which reactant was the limiting reactant in each trial? 6. Which reactant was in excess in each trial? 7. What was the theoretical yield, in moles, of CO 2 for the reaction that utilized 3.00 g of sodium bicarbonate? 8. One mole of gas at STP (standard temperature and pressure) has a volume of 22.4 L, what volume of CO 2 was produced in the reaction that utilized 3.00 g of sodium bicarbonate?
Background image of page 2
Answer Key: 1.) Answers will vary 2.) Answers will vary 3.) The balloon with 3.00 g of NaHCO 3 will inflate the fastest
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Background image of page 4
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}