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Justin Roth College ID: 0360782 Thomas Edison State College General Chemistry I (CHE-111) Section no.4 Semester and year: January 2016 Written...

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Name: Justin Roth College ID: 0360782 Thomas Edison State College General Chemistry I (CHE-111) Section no.:4 Semester and year: January 2016 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: (b) chemical reaction, (c) reactant, (d) product. (12 points) a.H2+O2=H2O b. Hydogen and Oxygen joined together to form Water. c. Hydrogen and Oxygen are the starting substances in the chemical reaction. d. H2O is formed from the reaction 2. Balance the following equations: (18 points) a. C + O 2 CO2 b. CO + O 2 2CO 2 c. Na + H 2 O H 2 +2NaOH d. Zn + HCl ZnCl 2 + H 2 e. 2NaOH+H2SO4 2H2O+Na2SO4 f. 2NH3+3CuO→ 3Cu+N2+3H2O 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) 2AI+3I2=2AII3 3x0.756=2.268 20.4/26.98=.756 moles 2.268x 126.9 =287g (Reference: Chang 3.47) 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 2 (g) SO 2 (g) How much sulfur (in tons), present in the original materials, would result in that quantity of SO 2 ? (5 points) 1.3x10^7tons S (Reference: Chang 3.69) 1
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5. Each copper(II) sulfate unit is associated with five water molecules in crystalline opper(II) sulfate pentahydrate (CuSO 4 5H 2 O). When this compound is heated in air above 100 o C, it loses the water molecules are also its blue color: .300 mol H2O If 9.60 g of CuSO 4 are left after heating 15.01 g of the blue compound, calculate the number of moles of water originally present in the compound. (5 points) 63.546+32.026+4x16+5(2 x1.01+16)= 249.711/16 5(15.01/9.60)=7.86 moles (Reference: Chang 3.73) 6. The fertilizer ammonium sulfate [(NH 4 ) 2 SO 4 ] is prepared by the reaction between ammonia (NH 3 ) and sulfuric acid: 2 NH 3 ( g ) + H 2 SO 4 ( aq ) (NH 4 ) 2 SO 4 ( aq ) How many kilograms of NH 3 are needed to produce 1.00 × 10 5 kg of (NH 4 ) 2 SO 4 ? (5 points) (1.00e5 kg (NH4)2SO4 / 1) * (1000 g (NH4)2SO4 / 1 kg (NH4)2SO4) * (1 mol (NH4)2SO4 / 132.1402 g (NH4)2SO4) * (2 mol NH3 / 1 mol (NH4)2SO4) * (17.031 g NH3 / 1 mol NH3) * (1 kg NH3 / 1000 g NH3) = 25777.16698 kg NH3. (Reference: Chang 3.77) 7. Nitric acid (NO) reacts with oxygen gas to form nitrogen dioxide (NO 2 ), a dark brown gas: 2NO( g ) + O 2 ( g ) → 2NO 2 ( g ) In one experiment 0.886 mole of NO is mixed with 0.503 mol of O 2 . a. Calculate which of the two reactants is the limiting reagent. (5 points). NO b. Calculate also the number of moles of NO 2 produced. (5 points) .886 mol NO2 is produced c. What reactant is left over and how much of it is left over? (5 points) 1.92g O2 (Reference: Chang 3.83) 2
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a. C + O2 → CO answer- 2C + O2 → 2CO b. CO + O2 → CO2 answer - 2CO + O2 → 2CO2 c. Na + H2O... View the full answer

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