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timofeeve [1]
2 years ago
11

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?
Chemistry
1 answer:
REY [17]2 years ago
5 0

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


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Answer:

v = 2,66x10⁻⁵ P[H₂C₂O₄]

Explanation:

For the reaction:

H₂C₂O₄(g) → CO₂(g) + HCOOH(g)

At t = 0, the initial pressure is just of H₂C₂O₄(g). At t= 20000 s, pressures will be:

H₂C₂O₄(g) = P₀ - x

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3rd point:

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That means law is:

v = 2,66x10⁻⁵ P[H₂C₂O₄]

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4 0
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