Chemistry Calculations PDF
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This document contains chemistry calculations, including problems and solutions for topics like molarity, molality, and vapor pressure. The calculations involve various chemical concepts including solution composition.
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### ID: 111542 ### Group - 3A 1. Mass NaCl = 6.87 g Mass Water = 100 g Mass of Solute Total Mass of Solution * 100 = 6.428 % = 6.87 / (100 + 6.87) * 100 2. X Glucose = 0.350 X Water = 0.650 Mol Solution = 100 Water = H<sub>2</sub>o = 2 + 16 = 18 Moles of Glucose...
### ID: 111542 ### Group - 3A 1. Mass NaCl = 6.87 g Mass Water = 100 g Mass of Solute Total Mass of Solution * 100 = 6.428 % = 6.87 / (100 + 6.87) * 100 2. X Glucose = 0.350 X Water = 0.650 Mol Solution = 100 Water = H<sub>2</sub>o = 2 + 16 = 18 Moles of Glucose = 0.350 * 100 = 35 mole Moles of Water = 0.650 * 100 = 65 mole Mass of Water = 65 * 18 = 1170 g Molarity of Glucose = Mass of Glucose / Mass of Water * 1000 = 35 / 1170 = 29.914 M ### 3. HNO<sub>3</sub> = 68% (MWt of HNO<sub>3</sub> = 68) Density = 1.504 g/ml Mass = Density * Volume = 1.504 * 1000 = 1504 g Mass of HNO<sub>3</sub> = 68 * 1504 = 1022. 729 g Moles of HNO<sub>3</sub> = Mass of HNO<sub>3</sub> / Molecular Weight of HNO<sub>3</sub> = 1022.729 / 68 = 15.04 mol Moles of HNO<sub>3</sub> / Volume = 15.04 / 1 = 15.04 mol ### 4. Mass of Glucose = 10 g Molecular Weight = 180 Solution = 100 g Mass of Glucose = 10/100 * 100 = 10 g Mass of Water = 100 - 10 = 90 g Moles of Glucose = Mass / Molar Mass = 10 / 180 = 0.0556 mol Mass of Water = 90 g Molality = Mass of Solute / Mass of Solvent = 0.0556 / 0.09 = 0.617 M ### 5. W+% = 0.9 * 1200 = 1080 g Solvent n<sub>Soln</sub> = W<sub>t</sub>/M.W<sub>t</sub> = 1080 / 18 = 60 X = n <sub>Soln</sub> / N<sub>total</sub> = 60 / 60 + 0.667 ### 6. n = W<sub>t</sub>/M.W<sub>t</sub> = 2226 / 62 = 3.59 mol M = n/W<sub>t</sub>(kg) = 3.59 / 200 x 10<sup>-3 </sup> = 17.95 M ### 7. n<sub>P</sub> = 252 / 72 = 3.5 mol n<sub>P</sub> = 1400 / 100 = 14 mol n<sub>T</sub> = 14 + 3.5 = 17.5 X<sub>P</sub> = n<sub>P</sub> / n<sub>T</sub> = 14 / 17.5 = 0.8 P<sub>T</sub> = X<sub>A</sub> P<sub>A</sub><sup>o</sup> + (1-X<sub>A</sub>)P<sub>B</sub><sup>o</sup> = 0.2 * 920 + (1-0.2) * 36 = 112.8 mmHg ### 8. P<sub>B</sub> = X<sub>B</sub> * P<sub>B</sub><sup>o</sup> = 0.7 * 75 = 52.5 mmHg P<sub>Total</sub> = X<sub>A</sub> * P<sub>A</sub><sup>o</sup> + X<sub>B</sub> * P<sub>B</sub><sup>o</sup> = 0.3*22 = 6.6 mmHg P<sub>T</sub> = 52.5 + 6.6 = 59.1 X<sub>B</sub> = P<sub>B</sub> / P<sub>T</sub> = 52.5 / 59.1 ### 9. ΔP = P<sub>i</sub><sup>o</sup> - P<sub>i</sub> = 0.8 - 0.6 = 0.2 ΔP = X * P<sup>o</sup> > X = ΔP / P<sup>o</sup> = 0.2 / 0.8 = 0.25 ### 10. M = DTF / K<sub>f</sub> = 1.5 / 3.9 = 0.384 n = M * W<sub>t</sub>(kg) = 0.384 * 75 * 10<sup>-3</sup> = 0.0288 mole W<sub>P</sub> = n * M.W<sub>t</sub> = 0.0288 * 176 = 5.089 ### 11. ΔT<sub>f</sub> = K<sub>f</sub> * m * Molality M<sub>2</sub> = No. of Solute / Wt of Solvent = n / Wt = 6.5 / 62 = 0.104 M = 0.104 / 200 x 10<sup>-3</sup> ### 12. ΔT<sub>f</sub> = T<sub>m</sub><sup>o</sup> - T<sub>m</sub> = 1.86 * 0.524 = 0.974 ### 13. C<sub>B</sub><sup>*</sup> = P<sub>B</sub><sup>*</sup> / P<sub>Total</sub> = 0.1086 / 2.3 C<sub>B</sub> = P<sub>B</sub> / P<sub>Total</sub> = 3.5 / 2.3 P = 93.7 atm
