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set 3 solns

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Department
Chemistry
Course
CH110
Professor
Quinn Major
Semester
Fall

Description
Practice Problems: Set #3-Solutions IIa) Balance the following equations:(10) 1) Zn (s) + H 3O 4aq) → Zn (PO3) (s4 2 H (g) 2 3Zn (s) + 2H P3 (a4) → Zn (PO ) 3s) 4 2 + 3H (2) 2. Mg N3(2) + H O (l2 → NH (g) + 3g(OH) (s) 2 Mg N3(s2 + 6H O2l) →2NH (g) 3 + 3Mg(OH) (s) 2 3. KMnO (aq4 + HCl(aq) → Cl (g) + M2O (s) + KCl(2q) + H O(l) 2 2 KMnO (a4) + 8HCl(aq) → 3Cl (g) 2 2 MnO (s) + 2 K2l(aq) + 4H 2(l) 4. NH 3g) + O (g2 → NO(g) + H O (l) 2 4NH (3) +5O (g) 2 4NO(g) + 6H O (l) 2 5. Al2S3(s) + H O (2) →Al(OH) 3 + H S2g) Al 2 3s) + 6H 2 (l) →42Al(OH) 3 + 3H 2(g) IIb) Write a balanced chemical equation for each of the following:(8) 1. Solid copper reacts with solid sulfur to form solid copper(I) sulfide. 2Cu(s) + S(s) →Cu S 2s) 2. Solid magnesium reacts with aqueous copper (I) nitrate to form aqueous magnesium nitrate and solid copper. Mg(s) + 2Cu (NO )aq3→ Mg(NO ) aq 3 2 + 2Cu(s) 3. Gaseous dinitrogen pentoxide decomposes to form nitrogen dioxide and oxygen gas. 2N 2 (5) →4NO 2 + O 2 4. Aqueous hydrochloric acid reacts with solid manganese (IV) oxide to form aqueous manganese (II) chloride, liquid water, and chlorine gas. 4HCl(aq) + MnO 2 → MnCl (a2) + 2H O2 + Cl 2g) IIIa) Write the chemical formula for each of the following(5) 1.Potassium Dichromate K Cr O 2 2 7 2. ammonium phosphate (NH ) PO 4 3 4 3. Phosphoric acid H3PO 4 4. Baking Soda NaHCO 3 5. Iron (III) sulfide Fe2S 3 Multiple Choice: 1. The balanced equation 2Cu(s) + O (g) → 2CuO(s) tells us that 1 mol of Cu 2 A. reacts with 1 mol of O2 B. produces one mol of CuO C. must react with 32g of O 2 D. cannot react with oxygen E. produces 2 mol of CuO 2. A 3.0 mol sample of KClO w3s decomposed according to the equation 2KClO (3) → 2KCl(s) + 3O (g)2 How many moles of O are2formed assuming 100% yield? A. 2.0 mol B. 2.5 mol C. 3.0 mol D. 4.0 mol E. 4.5 mol 3. What mass of carbon dioxide would be produced when 10.0 g of butane reacts with an excess of oxygen in the following reaction? 2C 4 10) + 13 O 2g) → 8CO (g2 + 10 H O(g) 2 A. 7.57g CO 2 B. 30.3g CO 2 C. 40.0g CO 2 D. 352g CO 2 E. none of these 4. How many molecules of carbon dioxide would be formed if 6.75g of propane is burned in the following reaction? C3H 8g) + 5O (g2 → 3 CO (g) 2 4H O (g) 2 23 A. 5.54 x 10 23lecules B. 1.39 x 10 molecules C. 20.3 x 10 molecules 23 D. 2.77 x 10 23 molecules E. 3.89 x 10 molecules 5. Consider the following reaction: 2A + B →3C + D 3.0 mol A and 2.0 mol B react to form 4.0 mol C. What is the percent yield of the reaction? A. 50% B. 67% C. 75% D. 89% E. 100% 6. When NH 3 is prepared from 28g N a2d excess H , t2e theoretical yield of NH 3s 34g. When this reaction is carried out in a given experiment, only 30g is produced. What is the percentage yield? A. 6% B. 12% C. 14% D. 82% E. 88% 7. The empirical formula for the compound having the formula H C O 2 2 4 is A. COH B. COH 2 C. C H2 2 D. C O2H4 2 E. CO H 2 8. Which of the following has the largest percent by mass of carbon? A. CaCO 3 B. CO 2 C. CH 4 D. NaHCO 3 9. A compound is analyzed and found to contain 12.1% carbon, 16.2% oxygen, and 71.7% chlorine (by mass). Calculate the empirical formula of this compound. A. COCl B. COCl 2 C. CO C2 D. CO C2 2 E. COCl 4 10. Calculate the molecular formula of a compound with the empirical formula CH O 2nd a molar mass of 150g/mol. A. C H2O4 2 B. C H3O6 3 C. C H4O8 4 D. C H5O10 5 E. C H6O12 6 11. A certain compound is found to have the percent composition (by mass) of 85.63% C and 14.37% H. The molar mass of the compound was found to be 42.0 g/mol. Calculate the empirical and the molecular formulas. A. C 2 a3d C H 4 6 B. CH and C H 3 3 C. CH a2d C H 3 6 D. CH and C H 3 2 6 E. C 2 a6d C H 3 9 12. The correct formula for arsenic(III) oxide is A. As 3 3 B. As 2 3 C. As 3 2 D. AsO E. As 3 13 . Identify the incorrect statement among the following: A. A mole is that quantity o
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