Name: Gas Laws Lab instructor may ask you to answer these in your lab notebook,

Question

Name: Gas Laws Lab instructor may ask you to answer these in your lab notebook, or to answer directly on this page and tun it in, or to include these answers in a formal lab report. Folow your instructor's directions. 1. According to the chemical reaction, if excess acetic acid is mixed with 6.0 g sodium bicarbonate, how many moles of CO2 produced? 2. What is the volume of carbon dioxide obtained if 0.15 g CO2 are produced in the reaction of acetic acid and sodium bicarbonate? Assume the temperature of 25.0°C and atmospheric pressure of 1.0 atm of pressure. 3. If your percentage was less than 100%, explain where you think the loss of carbon dioxide went? 4. Which method for collecting the gas is more efficient? Briefly explain. How would you improve these experiments to obtain more reliable data? 6

Explanation / Answer

Q1

CH3COOH + NaHCO3 = NaCH3COO + H2O + CO2

ratio is 1:1

mol of NaHCO3 = Mass/Mw = 6/84.007 = 0.071422 mol of NaHCO3

then,

mol of CO2 = 0.071422

q2

volume of

m = 0.15 g of CO2 produed

PV = nRT

V = nRT/P = (0.15/44)(0.082)(25+273)/1

V = 0.0833 L or 83.3 mL

Q3

if it is less, then CO2(g) migh have been gone to the auqeous solution, in order to form:

CO2(g) + H2O(l) = H2CO3(aq)

q4

typically, the trap between vapor and water will work the best, since the vapor is not likely to go into solution given those P, T conditions

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