Please solve # 4 and # 11. Also, if you would solve other questions, you could d

Question

Please solve # 4 and # 11. Also, if you would solve other questions, you could do that. I will really appreciate it if you solve other questions.

3. Describe how I would prepare a 500mL solution of 1.5 molar HC1 from a stock solution of concentrated 18M HC1. 4. If I add 10 grams of iron to 250mL of 0.132M ZnNO3)2 solution, what concentration of Fe(NO3)2 solution can I expect to form, assuming the volume of the solution is constant? 5. Why do gases exert pressure? 6. Explain how a closed tube manometer measures pressure draw a picture if necessary). 7. If I capture 56L of an unknown gas over water at 25°C and 745 mmHghow many moles of gas did I collect? 8. IfI fill my tire with air inside my garage at 75°F to a pressure of 36 psi, what will the partial pressure due to Nitrogen be when I drive outside on a freezing day of 3°F? 9. What would the density of Neon gas be at 30°C and 1 .02 atm? travel 10. How fast does an average molecule of O29? 11. If 0.32mole of Ne gas, 0.25 mole of N2 gas, and 020 mole of He gas, are mixed and the pressure is found to be 1.30 atm at 300K, what is the partial pressure of each gas and what is the volume each gas occupies?

Explanation / Answer

Ans 4 :

The reaction is given as :
Fe + Zn(NO3)2 = Fe(NO3)2 + Zn

Number of moles of iron available = 10/55.845 = 0.179 moles

Number of moles of Zn(NO3)2 = 0.132 x 0.250 = 0.033 moles

So Zn(NO3)2 is the limiting reagent.

Number of moles of Fe(NO3)2 formed will be : 0.033 moles

Volume = 250 mL

So the concentration of Fe(NO3)2 = 0.033 / 0.250

= 0.132 M

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