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

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: