Answer:
14.23g of (NH4)2CO3
Explanation:
We'll begin by writing the balanced equation for the reaction.
(NH4)2CO3 –> (NH4)2O + CO2
Next,, we shall determine the mass of (NH4)2CO3 that decomposed and the mass of CO2 produced from the balanced equation. This is illustrated below:
Molar mass of (NH4)2CO3 = 2[14+(4x1)] + 12 + (16x3)
= 2[14 +4] + 12 + 48
= 2[18] + 60 = 96g/mol
Mass of (NH4)2CO3 from the balanced equation = 1 x 96 = 96g
Molar mass of CO2 = 12 + (2x16) = 44g/mol
Mass of CO2 from the balanced equation = 1 x 44 = 44g.
Summary:
From the balanced equation above,
96g of (NH4)2CO3 decomposed to produce 44g of CO2.
Finally, we can determine the mass of (NH4)2CO3 that decomposed to produce 6.52g of CO2 as follow:
From the balanced equation above,
96g of (NH4)2CO3 decomposed to produce 44g of CO2.
Therefore, Xg of (NH4)2CO3 will decompose to produce 6.52g of CO2 i.e
Xg of (NH4)2CO3 = (96 x 6.52)/44
Xg of (NH4)2CO3 = 14.23g
Therefore, 14.23g of (NH4)2CO3 is needed to produce 6.52g of CO2.
