What is the mass of bismuth carbonate (597.99 g/mol) that decomposes to release 50.0ml of carbon dioxide gas at stp? 0.000445 g 0.00400 g 0.445 g 1.33 g 4.00 g?

The mass of bismuth carbonate that decomposed is 0.445 g

calculation

write the equation for reaction

that is Bi2(CO3)3 → Bi2O3 +3 CO2

find the moles of of CO2 formed

At STP 1 mole of a gas = 22.4 L

what about 50 Ml

convert the Ml to Liters = 50/1000= 0.05 L

moles of CO2 formed is therefore= 1 mole x 0.05 L/22.4 l =2.232 x10^-3 moles

by use of reacting ratio between Bi(CO3)3 to CO2 which is 1:3 the moles of Bi(CO3)3 is = 2.232 x10^-3 x1/3= 0.744 x10^-4 moles of Bi(CO3)3

mass of Bi(CO3)3 = molar mass x number of moles

mass= 0.744 x10^-4 moles x 597.99 g/mol = 0.445 grams