Answer:
Option (C) is correct.
Explanation:
Decomposition reaction: [tex](NH_{4})_{2}CO_{3}\rightarrow 2NH_{3}+CO_{2}+H_{2}O[/tex]
Molar mass of [tex]CO_{2}[/tex] = 44.01 g/mol
No. of moles = (mass)/(molar mass)
So, 6.52 g of [tex]CO_{2}[/tex] = [tex]\frac{6.52}{44.01}[/tex] moles of [tex]CO_{2}[/tex] = 0.148 moles of [tex]CO_{2}[/tex]
According to balanced equation-
1 mol of [tex]CO_{2}[/tex] is produced from decomposition of 1 mol of [tex](NH_{4})_{2}CO_{3}[/tex]
So, 0.148 mol of [tex]CO_{2}[/tex] is produced from decomposition of 0.148 mol of [tex](NH_{4})_{2}CO_{3}[/tex]
Hence, option (C) is correct.
