11. Calculate the Bot maximum number of moles of hydrogen bonds that can form in
ID: 540489 • Letter: 1
Question
11. Calculate the Bot maximum number of moles of hydrogen bonds that can form in a sample of 68 num iqud ammonla, NiHi (Answer imoles) b. How many hydrogen bonds will be in 24 Liters of gaseous ammonia? (Answer: Omoles) 12. Hydrogen bonds in water: In one mole of solid ice, there are 2.0 moles of hydrogen bonds. a. Water at 0 °C only contains 1.8 moles of hydrogen bonds per mole of H20. If it takes 5.25 k to melt one mole of ice, calculate the energy required to break one mole of hydrogen bonds. (at home: calculate how much energy is required to break an individual hydrogen bond) Water at 100 °C has 1.6 moles of hydrogen bonds per mole of H20. Assuming that all the heat is used only to break hydrogen bonds, predict the value of AHvap in k]/mol of H20. (hint: how many hydrogen bonds remain in water vapor?) b. 3. For each group, circle the compound that has the highest boiling point. lustify your answers Group 1: He Al CH4 (CH,OH) N, H-bond s Grop 2: NI, BH, most electrons Group 3: NHExplanation / Answer
11) a) no of mol of NH3 taken = w/mwt = 68 /17 = 4 mol
1 mol NH3 Ccontains, 1 mol H-bonds.
answer: 4 moles
b) as NH3 gas is taken , in gaseous state the molecules are free from H-bonds.so that
answer: 0 moles
12)
a) 1 mole ice = 2.o mole H-bonds
1 mole water at 0 c = 1.8 mole H-bonds
no of mole of H-bonds broken per each mole conversion of ice to water conversion = 2-1.8 = 0.2 mole
energy consumed = 5.25 kj
so that,
0.2 mol H-bonds = 5.25 kj
1 mol H-bonds = 5.25/0.2 = 26.25 kj/mol
b) 1 mole water at 100 c = 1.6 mole H-bonds
1 mole water vapor at 100 c = 0 mole H-bonds.
so that,
DHvap = 26.25*1.6 = 42 kj/mol
3) group 1: Al - metal posses strong atomic attractions.
group 2: CH3OH - it is having H-bonds.
group 3: NI3 - more no of electrons.so that more london dispersion forces.
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