<p> Chemistry 11 Review Unit 6</p><p>Chemistry 11 Name ______Date ______Review of Unit 6 </p><p>1. Balance the following equations:</p><p> a. NO + H2O  NH3 + O2 </p><p> b. (NH4)2Cr2O7 + AlCl3  Al2(Cr2O7)3 + NH4Cl</p><p> c. C17H36 + O2  CO2 + H2O</p><p> d. Co + H2SO4  Co2(SO4)3 + H2</p><p> e. P4 + Cl2  PCl3</p><p> f. H3PO4 + Ba(OH)2  Ba3(PO4)2 + H2O</p><p> g. Al(CH3COO)3  Al + C + H2 + O2</p><p>2. Complete, balance and classify the following equations as synthesis, decomposition, single replacement, double replacement, neutralization or combustion. </p><p> a. Al + Zn(NO3)2 </p><p>Reaction Type ______</p><p> b. C6H14 + O2 </p><p>Reaction Type ______</p><p> c. Na3PO4 + Ca(NO3)2 </p><p>Reaction Type ______</p><p> d. Mg(H2PO4)2 </p><p>Reaction Type ______</p><p> e. Cl2 + KI </p><p>Reaction Type ______Chemistry 11 Review Unit 6</p><p> f. Al + F2 </p><p>Reaction Type ______</p><p> g. Zn + Cu(ClO3)2 </p><p>Reaction Type ______</p><p> h. Co(NO3)3 + (NH4)2C2O4 </p><p>Reaction Type ______</p><p> i. C12H25OH + O2 </p><p>Reaction Type ______</p><p> j. Sr(OH)2 + HNO3 </p><p>Reaction Type ______</p><p> k. V + O2 </p><p>(Assume combining capacity of V is 5+)</p><p>Reaction Type ______</p><p> l. Rb3AsO4 </p><p>Reaction Type ______</p><p> m. CsOH + H3PO4 </p><p>Reaction Type ______</p><p> n. Ni(NO3)2 + (NH4)3PO4 </p><p>Reaction Type ______</p><p> o. Al + H2CO3 </p><p>Reaction Type ______</p><p> p. MgSO4 + AgNO3 </p><p>Reaction Type ______Chemistry 11 Review Unit 6</p><p>3. State whether each of the following are exothermic or endothermic. </p><p> a. HCl + 432 kJ  H + Cl Answer ______</p><p> b. C12H22O11 + 12 O2  12CO2 + 11H2O + 5638 kJ Answer ______</p><p> c. H2O(l)  H2O(g) Answer ______</p><p> d. A + B ) J k (</p><p> y g r e AB n E Reaction Proceeding </p><p>Answer ______</p><p> e. C + D  CD H= +65.7 kJ Answer ______</p><p> f. E + F  G + H= - 437 kJ Answer ______</p><p>4. In an exothermic reaction, the surroundings get (warmer/cooler) ______.</p><p>5. Define enthalpy </p><p>6. Why does a light stick glow brighter when it is heated?</p><p>7. Which reaction will be faster? 6M HCl with zinc or 3 M HCl with zinc </p><p>8. Does concentration increase the rate of reaction A or B. Reaction A 2Na(s) + SrCrO4(s) → Sr(s) + Na2CrO4(s) Reaction B Ba(OH)2 (g) + MgCl2(aq) → Mg(OH)2(aq) + BaCl2(aq) 9. How does surface area affect reaction rate? Give an example of a reaction that IS NOT affected by surface area. Chemistry 11 Review Unit 6</p><p>10. Use the following Potential Energy Diagram to answer the questions below: 100</p><p>ABC 80 ) J k ( 60 y AB + C g r e n E l a i 40 t n e t o P A + BC 20</p><p>0 Progress of Reaction</p><p> a) Determine the Activation Energy for the forward reaction... ______kJ</p><p> b) Determine the Activation Energy for the reverse reaction.... ______kJ</p><p> c) What is the Enthalpy Change (H) for the forward reaction?.. ______kJ</p><p> d) What is the Enthalpy Change (H) for the reverse reaction?.. ______kJ</p><p> e) The forward reaction is ______thermic.</p><p> f) The reverse reaction is ______thermic.</p><p> g) Which species or set of species forms the Activated Complex? ______</p><p> h) What is the formula for the activated complex? ______</p><p>11. State the meaning of Activation Energy Chemistry 11 Review Unit 6</p><p>12. Use the following Potential Energy Diagram to answer the questions below:</p><p>Potential Energy ABC 300</p><p>250</p><p>200 A + BC 150</p><p>100 AB + C 50</p><p>0 0.0 0.2 0.4 0.6 0.8 1.0 1.2 Progress of Reaction</p><p> a) Determine the Activation Energy for the forward reaction... ______kJ</p><p> b) Determine the Activation Energy for the reverse reaction.... ______kJ</p><p> c) What is the Enthalpy Change (H) for the forward reaction?..______kJ</p><p> d) What is the Enthalpy Change (H) for the reverse reaction?..______kJ</p><p> e) The forward reaction is ______thermic.</p><p> f) The reverse reaction is ______thermic.</p><p> g) Which species or set of species forms the Activated Complex? ______</p>