Written Assignment 4.docx - Thomas Edison State University General Chemistry I with Labs(CHE-121 Section no Semester and year January-2020 Written

Written Assignment 4.docx - Thomas Edison State University...

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Thomas Edison State University General Chemistry I with Labs (CHE-121) Section no.: Semester and year: January-2020 Written Assignment 4: Chemical Reactions Answer all assigned questions and problems, and show all work. 1. Write the (a) balanced equation for the formation of liquid water from hydrogen and oxygen gas, and use it to explain the following terms: a. chemical reaction, b. reactant, c. product. (12 points) Balanced equation of this reaction : 2H 2 (g) + O 2 (g) → 2H 2 O (l) Chemical Reaction : 2 moles of H 2 react with 1 mole of O 2 and process 2 mole of H 2 O (Water). Reactant : Reactant can be explained as substance that take part in and undergoes change during a reaction. Here reactant are H 2 and O 2 . Product : Product can be explained as species form from the chemical reaction. In this case water H 2 O produced after chemical reaction between H 2 and O 2. 2. Balance the following equations: (18 points) a. C + O 2 CO => 2C + O 2 → 2CO b. CO + O 2 CO 2 => 2CO + O 2 → 2CO 2 c. Na + H 2 O → H 2 + NaOH => 2Na + 2H 2 O → H 2 + 2NaOH d. Zn + HCl → ZnCl 2 + H 2 => Zn + 2HCl → ZnCl 2 + H 2 e. NaOH + H 2 SO 4 H 2 O + Na 2 SO 4 => 2NaOH + H 2 SO 4 H 2 O + Na 2 SO 4 f. NH 3 + CuO → Cu + N 2 + H 2 O => 2NH 3 + 3CuO → 3Cu + N 2 + 3H 2 O 3. Calculate the mass in grams of iodine (I 2 ) that will react completely with 20.4 g of aluminum (Al) to form aluminum iodide (AlI 3 ). (5 points) (Reference: Chang 3.47) The balanced chemical reaction between Aluminium and Iodine is, 2 Al (s) + 3 I 2 (s) → 2AlI 3 (s) Mass of Aluminium is 20.4 g and molecular mass of Al is 26.98 Moles of Aluminium = 20.4 / 26.98 = 0.756 mol The stoichiometric mole ratio of iodine to Al = 3 mol of I 2 2 molof Al
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Moles of iodine that is react with 0.756 mol of Al is = 0.756 3 2 = 1.134 mole I 2 Molecular mass of I 2 is 253.808 g/mole Mass of I 2 required for require for this reaction = 253.808 * 1.134 = 287.81g 4. The annual production of sulfur dioxide from burning coal and fossil fuels, auto exhaust, and other sources is about 26 million tons. The equation for the reaction is S(s) + O
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