## (Solved) Hi! Thank you for answering the questions I have posted! I like

Hi!  Thank you for answering the questions I have posted!  I like that you physically write them on paper and attach them as a file so I can see how you are doing them.  If you can help me with a lab that I have due I'd greatly appreciate it!!!!!!!

The lab was in late nite labs on The Molar Mass of Magnesium.  I tried to search for it on here to see if someone had already done it but apparently no one had.....

Below are the measurements taken:

NOTES:

Took a 150 mL Erlenmeyer flask and added 10 mL of water and 10 mL of 6m HCl.

Measured temp= 21.5 C

Measured Volume- 150-20= 130

Pressure - 1 atm

Then added 0.1 g of Mg- It began bubbling and the temp 7 pressure went up.

Temp= 31C

Pressure= 1.82

Placed a gas syringe- V=101.6

Final Temp- 23.4

Final Pressure= 1.77

These are the questions:

Write a balanced equation for the reaction of Mg with Hcl.

Record the volume, pressure, and temperature of the gas in the flask before the addition of the Magnesium.

Use the ideal gas equation PV=nRT to find the number of moles.  The gas constant R is 0.082057 (L*atm) (K*mole)  Convert temp to Kelvin by adding 274

Use the balanced equation for the reaction to convert moles of hydrogen gas to moles of Mg consumed in the reaction.

In This reaction, all of the magnesium reacts to completion, Given that 0.004 moles of Mg was used to produce 0.004 mol of Hydrogen gas.  What is the molar mass of Mg?  Use the mass of Mg added to the reaction.  (molar mass=mass/moles)

I'm taking this class online and it's SO hard!!!!  I haven't taken Chemistry since High school and that was a really really REALLY long time ago......

Took a 150 mL Erlenmeyer flask and added 10 mL of water and 10 mL of 6m HCl.

Measured temp= 21.5 C

Measured Volume- 150-20= 130

Pressure - 1 atm

Then added 0.1 g of Mg- It...

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This question was answered on: Oct 15, 2019

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