14.
Correct option: a
Mass of LiOH = 1.00 kg = 1000 g
Molar mass of LiOH = 23.95 g/mol
Moles of LiOH = 1000 g/23.95 g/mol = 41.8 mol
Balanced equation:
2LiOH + CO2Li2CO3 + H2O
Theoretically, 2 mol of LiOH absorb 1 mol of CO2
Therefore, 41.8 mol of LiOH absorb = (1 mol/2 mol) x 41.8 mol = 20.9 mol of CO2
Molar mass of CO2 = 44 g/mol
Hence, the mass of CO2 can be absorbed = 20.9 mol x 44 g/mol = 920 g
17.
Correct option: c
Mass of butane = 100 g
Molar mass of butane = 58.12 g/mol
Moles of butane = 100 g/ 58.12 g/mol = 1.72 mol
Mass of oxygen = 100 g
Molar mass of oxygen = 32 g/mol
Moles of oxygen = 100 g/ 32 g/mol = 3.12 mol
2C4H10 + 13O2 → 8CO2 + 10H2O
For complete reaction, the required mole ratio of butane : O2 = 2 : 13
The available mole ratio of butane : O2 = 1.72 : 3.12
= 1 : 1.8
= 2 : 3.6
Thus, per mol of butane, the available mol of O2 is less than required.
Hence, butane is the limiting reagent in the reaction.
Theoretically, 2 mol of butane yields 8 mol of CO2
Therefore, 1.72 mol of butane yields = (8 mol/2 mol) x 1.72 mol = 6.88 mol of CO2
Molar mass of CO2 = 44 g/mol
Hence, the theoretical yield of CO2 = 6.88 mol x 44 g/mol = 303 g
Actual yield of CO2 = 50.0 g
Percent yield = (50.0 g/303 g) x 100 = 16.5 %
18.
Correct option: c
Balanced molecular equation:
Fe(NO3)3(aq) + 3KOH(aq) Fe(OH)3(s) + 3KNO3(aq)
The complete ionic equation:
Fe3+(aq) + 3NO3-(aq) + 3K+(aq) + 3OH-(aq) Fe(OH)3(s) + 3K+(aq) + 3NO3-(aq)
Hence, the coefficient in front of nitrate ion = 3
I need help with Questions 14, 17, and 18. Please show work! of 6 + ......
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