Question

Free Response For questions A and B. A hydrocarbon containing 83.9% of carbon and 16.1% of hydrogen was burned in a rigid, enclosed box with the pressure of 715 mmHg at 55°C and an oxygen volume of 5090 ml. At the end of the reaction, the temperature cooled down to 0°C. Molar mass of the hydrocon is 100.2 g/mol. A. What is the amount of O2 reacted in gram. B. What is the yield of H20, in grams, after the reaction has completed?

Answer 1

mass of Hydrgen Now ) Molar mass of hydro Carbon is = 100.2 g/mol atomic mass of Carbon = 12 g atomic mass of ox xygen - 16 g atomic G IN 83.9%. Carbon in 100.2 g hydrocarbon = 83.9 x 100.2 g = 84.06 Carbon So number of by Carbon atom in the hydro Carbon = 84.06 g Lg = 7 Again, Hydrogen in 100.2 g hydrocarbon - 1601 x 100.2 g = 16.13 g Hydrogen So, number of hydrogen atom in the hydro Carbon - 16:13 g 16.1% 100 1 - 16 So, the molecular formula of hydro Carbon = Ghib HIGH (heptane) Now, the chemical reaction is Gytis + 11 L 7 COL + 8 H₂O volume of O2 gas used - 5090 ml = 5.09 Lit. density of or gas at STP = 1.429 g/lit So, 02 gas woed in gram = 5:09 bit x 1.429 g = 7.27 gram: - 7.27 g Awower. Lif g So, oxygen react in

from the balanced equation we need 352 g 02 gard Topo 200 g hydro Carbon for fully Commission But actually used f. 27g O2 gars, but no hydrocarbon remain, se hydro Carbon used Small amount Like 3529 02 O2 fully react with 7.27 go fully react with 100.2 x 7.27 g 100.2 g G H16 352 2.06 g GHIG So, the used 2 2.06 g Again, from 100.2 100.2 g Ghil we get 144 g Ho From, 2.06g Ghis we get 144 X 2.06 100.2 g Ro a Note :- 2.96 g ho Answer. & density of oxygen Collected from internet. & molecular beight of H₂O = 18 g 8 molecule tho is formed , so (8+18) A g es molecular weight of a = 32 11 moleure of a needed so (11832) g According 2 144 oblanced egnication 2 35 Lg