General Chemistry homework Chapter 4,5,6

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I want you to do all the questions correctly and with steps. Thank you for tour time. Do your best , I want to get 100. Show your work and make it simple because I want to understand it. Make it short if you can , but you need to show work. thanks

NATSCI 211_Summer 2018 Homework Set #2 Due: June 28, 20178 100 Points 1. Predict the precipitate produced by mixing an Al(NO3)3 solution with a NaOH solution. Write the net ionic equation for the reaction. 2. Which of the following processes will likely result in a precipitation reaction? (a) Mixing a NaNO3 solution with a CuSO4 solution. (b) Mixing a BaCl2 solution with a K2SO4 solution. Write a net ionic equation for the precipitation reaction. 3. How would you prepare 60.0 mL of 0.200 M HNO3 from a stock solution of 4.00 M HNO3? 4. How many grams of NaCl are required to precipitate most of the Ag+ ions from 2.5 X 102 mL of 0.0113 M AgNO3? Write the net ionic equation for the reaction. 5. Iron(II) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic equation: Cr2O7-2 + 6 Fe+2 + 14 H+ → 2 Cr+3 + 6 Fe+3 + 7 H2O If it takes 26.0 mL of 0.0250 M K2Cr2O7 to titrate 25.0 mL of a solution containing Fe+2, what is the molar concentration of Fe+2. 6. A 6.22 kg piece of Copper metal is heated from 20.5°c to 324.3°C. Calculate the heat absorbed (in kJ) by the metal. 7. Compare the bond enthalpy of F2 with the energy change for the following process: F2(g) → F+(g) + F-(g) Which is the preferred dissociation for F2, energetically speaking? (Specifics!!!) 8. The first step in the industrial recovery of Zn from the zinc sulfide ore is roasting, that is, the conversion of ZnS to ZnO by heating: 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2(g) ∆H = -879 kJ/mol Calculate the heat evolved (in kJ) per gram of ZnS roasted. 9. A piece of sodium metal reacts completely with water as follows: 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) The hydrogen gas generated is collected over water at 25.0°C. The volume of the gas is 246 mL measured at 1.00 atm. Calculate the number of grams of sodium used in the reaction. (Vapor pressure of water at 25°C = 0.0313atm). 10. A 2.14 L sample of HCl gas at 2.61 atm and 28°C is completely dissolved in 668 mL of water to form hydrochloric acid solution. Calculate the molarity of the acid solution. Assume no change in volume. 11. Calculate the work done in joules when 1.0 mole of water vaporizes at 1.0 atm and 100°C. Assume that the volume of liquid water is negligible compared with that of steam at 100°C, and ideal gas behavior. 12. Ozone molecules in the stratosphere absorb much of the harmful radiation from the sun. Typically, the temperature and pressure of ozone in the stratosphere are 250 K and 1.0 X 10-3 atm, respectively. How many ozone molecules are present in 1.0 L of air under these conditions? 13. Calculate the standard enthalpy of formation of liquid methanol, CH3OH(l), using the following information: 14. At 25°C, the following heats of reaction are known: At the same temperature, use the above data to calculate the heat released (kJ) when 3.40 moles of ClF(g) reacts with excess F2: ClF(g) + F2(g) →ClF3(g) 15. A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases.
100 Points 1. Predict the precipitate produced by mixing an Al(NO3)3 solution with a NaOH solution. Write the net ionic equation for the reaction. 2. Which of the following processes will likely result in a precipitation reaction? (a) Mixing a NaNO3 solution with a CuSO4 solution. (b) Mixing a BaCl2 solution with a K2SO4 solution. Write a net ionic equation for the precipitation reaction. 3. How would you prepare 60.0 mL of 0.200 M HNO3 from a stock solution of 4.00 M HNO3? 4. How many grams of NaCl are required to precipitate most of the Ag+ ions from 2.5 X 102 mL of 0.0113 M AgNO3? Write the net ionic equation for the reaction. 5. Iron(II) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic equation: Cr2O7-2 + 6 Fe+2 + 14 H+ → 2 Cr+3 + 6 Fe+3 + 7 H2O If it takes 26.0 mL of 0.0250 M K2Cr2O7 to titrate 25.0 mL of a solution containing Fe+2, what is the molar concentration of Fe+2. 6. A 6.22 kg piece of Copper metal is heated from 20.5°c to 324.3°C. Calculate the heat absorbed (in kJ) by the metal. 7. Compare the bond enthalpy of F2 with the energy change for the following process: F2(g) → F+(g) + F-(g) Which is the preferred dissociation for F2, energetically speaking? (Specifics!!!) 8. The first step in the industrial recovery of Zn from the zinc sulfide ore is roasting, that is, the conversion of ZnS to ZnO by heating: 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2(g) ∆H = -879 kJ/mol Calculate the heat evolved (in kJ) per gram of ZnS roasted. 9. A piece of sodium metal reacts completely with water as follows: 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) The hydrogen gas generated is collected over water at 25.0°C. The volume of the gas is 246 mL measured at 1.00 atm. Calculate the number of grams of sodium used in the reaction. (Vapor pressure of water at 25°C = 0.0313atm). 10. A 2.14 L sample of HCl gas at 2.61 atm and 28°C is completely dissolved in 668 mL of water to form hydrochloric acid solution. Calculate the molarity of the acid solution. Assume no change in volume. 11. Calculate the work done in joules when 1.0 mole of water vaporizes at 1.0 atm and 100°C. Assume that the volume of liquid water is negligible compared with that of steam at 100°C, and ideal gas behavior. 12. Ozone molecules in the stratosphere absorb much of the harmful radiation from the sun. Typically, the temperature and pressure of ozone in the stratosphere are 250 K and 1.0 X 10-3 atm, respectively. How many ozone molecules are present in 1.0 L of air under these conditions? 13. Calculate the standard enthalpy of formation of liquid methanol, CH3OH(l), using the following information: 14. At 25°C, the following heats of reaction are known: At the same temperature, use the above data to calculate the heat released (kJ) when 3.40 moles of ClF(g) reacts with excess F2: ClF(g) + F2(g) →ClF3(g) 15. A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases.

Tutor Answer

Robertmariasi
School: University of Virginia

Hello there,Just wanted to inform you that I managed to finish your task as I promised. I usually finish my task a lot faster but this time I was sleeping when I was assigned. Anyway, it seems like I am still 2 hours and a half ahead of the deadline ...

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Anonymous
Top quality work from this guy! I'll be back!

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