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set 3

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Department
Chemistry
Course
CH110
Professor
Quinn Major
Semester
Fall

Description
Practice Problems set: Set #3 IIa) Balance the following equations:(10) 1) Zn (s) + H PO (aq)  Zn (PO ) (s) + H (g) 3 4 3 4 2 2 2. Mg N (s) + H O (l)  NH (g) + Mg(OH) (s) 3 2 2 3 2 3. KMnO (aq)4+ HCl(aq)  Cl (g) + MnO 2s) + KCl(aq) +2H O(l) 2 4. NH (g)3+ O (g) 2 NO(g) + H O (l) 2 5. Al2 3(s) + H O (2)  Al(OH) + H S(g3 2 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. 2. Solid magnesium reacts with aqueous copper (I) nitrate to form aqueous magnesium nitrate and solid copper. 3. Gaseous dinitrogen pentoxide decomposes to form nitrogen dioxide and oxygen gas. 4. Aqueous hydrochloric acid reacts with solid manganese (IV) oxide to form aqueous manganese (II) chloride, liquid water, and chlorine gas. IIIa) Write the chemical formula for each of the following(5) 1.Potassium Dichromate ------------------ 2. ammonium phosphate ------------------ 3. Phosphoric acid ------------------ 4. Baking Soda -------------------- 5. Iron (III) sulfide --------------------- Multiple Choice: 1. The balanced equation 2Cu(s) + O (g) 22uO(s) tells us that 1 mol of Cu A. reacts with 1 mol of O 2 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 was 3ecomposed according to the equation 2KClO (3)  2KCl(s) + 3O (g) 2 How many moles of O are 2ormed 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 H (g) + 13 O (g)  8CO (g) + 10 H O(g) 4 10 2 2 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? C 3 8g) + 5O (g2  3 CO (g) 2 4H O (g) 2 A. 5.54 x 10 molecules 23 B. 1.39 x 10 molecules 23 C. 20.3 x 10 mo23cules D. 2.77 x 10 molecules 23 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 is3prepared from 28g N and2excess H , th2 theoretical yield of NH is334g. 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 is 2 2 4 A. COH B. COH 2 C. C 2 2 D. C 2 4 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 2l D. CO 2l 2 E. COCl 4 10. Calculate the molecular formula of a compound with the empirical formula CH O2and a molar mass of 150g/mol. A. C H2O 4 2 B. C H3O 6 3 C. C H4O 8 4 D. C H5O 10 5 E. C H O 6 12 6 11. A certain compound is found to have the percent composition (by mass) of 85.6
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