2.1.7 Practice_ Chemical Reactions

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Chemistry

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Nov 24, 2024

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Tiffany Markovich 12/2/23 2.1.7 Practice: Chemical Reactions 1. Conditions around hydrothermal vents deep in the ocean floor can enable chemical reactions that produce solid materials. A student models one of these reactions by combining aqueous Ca(OH) 2 and Na 2 SO 4 , and observes the formation of a solid in a liquid. a. Justify the choice of a net ionic equation for describing this reaction. The precipitate forms and the remaining ions remain in the solution as shown by the net ionic equation. b. Write and balance a net ionic equation for the reaction. Show your original equation as well as the balanced one. Original equation: Ca(OH)2(aq) + Na2SO4(aq) → CaSO4(s) + 2NaOH(aq) Balanced equation: Ca2 + 2OH + 2Na + SO4^- 2 → CaSO4 +2Na + 2OH c. Explain the steps you took to balance the original unbalanced net ionic equation. You get the following: Ca2 + 2OH + 2Na + SO4^-2 → CaSO4 + 2Na + 2OH. Then, cancel out what is found on both sides of the equation to get the following: 2OH + 2Na 2. Identify the oxidation numbers for each element in the following equations. Then determine whether each equation describes a redox reaction. Justify your answer in terms of electron transfer. Describe the oxidation and reduction that occurs. a. Ca + 2HCl → CaCl 2 + H 2 - This a redox reaction - Oxidation: The atoms Ca is at zero charge: Ca + 2 in CaCI2 - It loses 2 electrons
- Reduction: 2H + 1 gains 2 electrons - H2 is at zero charge at each hydrogen atom b. 2KOH + K 2 Cr 2 O 7 → 2K 2 CrO 4 + H 2 O - This a redox reaction - Cr does not change - Each Cr in K2Cr2O7 has gained 6 electrons each in both K2CrO4 - There is no change for K+1, O-2, H+1 → K+1, O-2, H+1 c. AgNO 3 + KI → AgI + KNO 3 - This is not a redox reaction - Everything seems to be balanced d. 2PbS + 3O 2 → 2PbO + 2SO 2 - This is a redox reaction - S goes from -2 to +4 electrons - O goes from 0 to -2 - S goes through oxidation and O goes through reduction
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