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!
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
Regarding any doubt plz let me know..
I will explain
can you please explain part C again? how do i know the mass of the silver (i) carbonate that i started with?
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
I hope you understood
okay thank you for explaining!
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