Question

i need help filling out this table please

Balloon # Moles of gas that could in theory be produced Liters of gas that could in theory be produced % yield of gas produced -- show calc Show calculations for theoretical moles of gas and theoretical Liters of gas: [4.5pts]

Answer 1

We have following equation:

NaHCO₃ (aq) + CH₃COOH (aq) ---------------> CH₃COONa (aq) + CO₂ (g) + H₂O (l)

To calculate volume we can use ideal gas law :

PV = nRT (P = pressure, V= volume, T =absolute temp. , n= no. on moles , R =constant )

Your calculation for moles of acetic acid is incorrect , thus limiting reagent :

Acetic acid in vinegar is 0.8368 M= 0.8363 mol /L

thus moles of acetic acid used will be : (4.93 ml*0.8363mol/L) / 1000 ml

# 1 : 0.004 moles   # 2 : 0.004 moles   # 3 : 0.004 moles # 4 : 0.008 moles # 5 : 0.008 moles   # 6: 0.008 moles

1. Moles of gas in theory could produced

from balanced equation : 1 mol of NaHCO₃ = 1mol CH₃COOH = 1 mol of gas

moles of gas produced depends on moles of limiting reagent :

# 1 : 0.002 moles   # 2 : 0.004 moles   # 3 : 0.004 moles # 4 : 0.004 moles   # 5 : 0.002 moles   # 6: 0.007 moles

2. liters of gas in theory could produced

From PV = nRT : V = nRT / P

we have : P = 1 atm. ; n = no. of moles ; T = 337.15 K (as measured by you )

R = 0.082 L-atm / mol-K

# 1 : n = 0.002 moles   

V = (0.002 mole* 0.082 L-atm / mol-K *337.15 K )/ 1 atm = 0.0553 L

# 2 : n=0.004 moles

V = (0.004 mole* 0.082 L-atm / mol-K *337.15 K )/ 1 atm = 0.1106 L

  # 3 :n=0.004 moles

V = (0.004 mole* 0.082 L-atm / mol-K *337.15 K )/ 1 atm = 0.1106

   # 4 : n= 0.004 moles

  V = (0.004 mole* 0.082 L-atm / mol-K *337.15 K )/ 1 atm = 0.1106 L

# 5 : n = 0.002 moles

  V = (0.002 mole* 0.082 L-atm / mol-K *337.15 K )/ 1 atm = 0.0553 L

  # 6: n = 0.007 moles

   V = (0.007 mole* 0.082 L-atm / mol-K *337.15 K )/ 1 atm = 0.1935 L  

3. % yield of gas :

# 1 : actual yield = 0.0355 L

Theory yield = 0.0553 L ; % yield =  0.0355 L /0.0553 L *100 = 64.2 %

# 2 : actual yield = 0.0355 L

Theory yield = 0.1106 L ; % yield =  0.0355 L /0.1106 L  *100 = 32.1 %

  # 3 : actual yield = 0.0446 L

Theory yield = 0.1106 L ; % yield =  0.0446 L /0.1106 L  *100 = 40.3 %  

   # 4 : actual yield = 0.0477 L

Theory yield = 0.1106 L ; % yield =  0.0477 L /0.1106 L  *100 = 43.1 %

# 5 : actual yield = 0.0509 L

Theory yield = 0.0553 L ; % yield =  0.0509 L /0.0553 L  *100 = 92.0 %

# 6 : actual yield = 0.0654 L

Theory yield = 0.1935 L ; % yield =  0.0654 L /0.1935 L  *100 =33.8 %