chemistry help on decomposition?

Chemistry
Tutor: None Selected Time limit: 1 Day

Silver (i) carbonate was decomposed by heating 948 ml of CO2 gas, collected over water 19.0 celsius and a pressure of 748.6 mmHG. 

A) write a balanced equation for this reaction

b) calculate how many grams of  carbon dioxide were collected?

c) assuming all the silver (i) carbonate decomposed, what mass of silver (i) carbonate did you start with?

please explain, i really dont understand the steps to this problem! thank you!

Apr 26th, 2015

A) Ag2CO3 = Ag2O + CO2

b)  one mole of CO2 = 22.4L

 mole of CO2 produced =  0.948/22.4 = 0.042 mol 

  mass = 0.042 x molecular weight of CO2 = 0.042 x 44 = 1.848 g

C)                                 Ag2CO3 = Ag2O + CO2

    initial mole                      x                  0             0

 After decomposition         0                   x             x


Apr 26th, 2015

Regarding any doubt plz let me know..

 I will explain 

Apr 26th, 2015

can you please explain part C again? how do i know the mass of the silver (i) carbonate that i started with?

Apr 27th, 2015

ok.. you got   0.042 mol of CO2 = x 

X= 0.042 that will be mole of silver (i) carbonate

 Gram of silver (i) carbonate = 0.042 * molecular weight of silver (i) carbonate

                                               = 0.042 *275.74 = 11.58 g      

Apr 27th, 2015

I hope you understood 

Apr 27th, 2015

okay thank you for explaining!

Apr 27th, 2015

welcome here 

Apr 27th, 2015

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