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trapecia [35]
3 years ago
8

Bismuth oxide reacts with carbon to form bismuth metal: bi2o3(s) + 3c(s) → 2bi(s) + 3co(g) when 689 g of bi2o3 reacts with exces

s carbon, (a) how many moles of bi form? 2.957 mol bi (b) how many grams of co form? g co

Chemistry
2 answers:
ExtremeBDS [4]3 years ago
8 0
Using the answer from the first part, we know that 2.957 moles of bismuth have formed. Moreover, the molar ratio between bismuth and carbon monoxide is:

2 : 3

Using the method of ratios,

2 : 3
2.957 : CO

CO = (3 * 2.957) / 2
CO = 4.4355

4.436 moles of carbon monoxide will be formed
Hunter-Best [27]3 years ago
7 0

CO mass = 4,435. 18 = 79,839 grams

Stokiometry in Chemistry learns about chemical reactions mainly emphasizing quantitative, such as calculation of volume, mass, number, which is related to the number of ions, molecules, elements etc.

In chemical calculations, the reaction can be determined, the number of substances that can be expressed in units of mass, volume, mole, or determine a chemical formula, for example the substance level or molecular formula of hydrate.

In stockiometry therein includes

relative atomic mass (Ar) and relative molecular mass (Mr)

Mr. AxBy = (x.Ar A + y. Ar B)

Reactions that occur:

Bi₂O₃ (s) + 3C (s) → 2Bi (s) + 3CO (g)

  • We specify mole Bi₂O₃

Mr Bi₂O₃ = 2. ar bi + 3. Ar O

Mr Bi₂O₃ = 2. 209 + 3. 16

Mr. Bi₂O₃= 466

mole Bi₂O₃ = gram / Mr

mole = 689/466

mole 1.4785

  • A. Comparison of Bi reaction coefficients: Bi₂O₃ = 1: 2, then Bi moles = 2. 1,4785 = 2, 957

Comparison of Bi reaction coefficients:  Bi₂O₃  = 1: 2,

  • B. While the number of moles CO = 3 x 1.4785 = 4,435

Mr. CO = 12 + 16 = 18

mass CO = mole. Mr

CO mass = 4,435. 18 = 79,839 grams

<h3><em>Learn more </em></h3>

how many moles of water you can produce

brainly.com/question/1405182

Excess reactant

brainly.com/question/6857557

The percentage yield

brainly.com/question/12044319

Limiting reactant

brainly.com/question/5798341

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We have to write the balanced equation as,

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In which reaction does the oxidation number of hydrogen change? In which reaction does the oxidation number of hydrogen change?
dedylja [7]

<u>Answer:</u> The correct answer is 2Na(s)+2H_2O(l)\rightarrow 2NaOH(aq.)+H_2(g)

<u>Explanation:</u>

Oxidation number is defined as the number which is given to an atom when it looses or gains electron. When an atom looses electron, it attains a positive oxidation state. When an atom gains electron, it attains a negative oxidation state.

Oxidation state of the atoms in their elemental state is considered as 0. Hydrogen is present as gaseous state.

For the given chemical reactions:

  • <u>Reaction 1:</u>  2HClO_4(aq.)+CaCO_3(s)\rightarrow Ca(ClO_4)_2(aq.)+H_2O(l)+CO_2 (g)

Oxidation state of hydrogen on reactant side: +1

Oxidation state of hydrogen on product side: +1

Thus, the oxidation state of hydrogen is not changing.

  • <u>Reaction 2:</u>  CaO(s)+H_2O(l)\rightarrow Ca(OH)_2(s)

Oxidation state of hydrogen on reactant side: +1

Oxidation state of hydrogen on product side: +1

Thus, the oxidation state of hydrogen is not changing.

  • <u>Reaction 3:</u>  HCl(aq.)+NaOH(aq.)\rightarrow NaCl(aq.)+H_2O(l)

Oxidation state of hydrogen on reactant side: +1

Oxidation state of hydrogen on product side: +1

Thus, the oxidation state of hydrogen is not changing.

  • <u>Reaction 4:</u>  2Na(s)+2H_2O(l)\rightarrow 2NaOH(aq.)+H_2(g)

Oxidation state of hydrogen on reactant side: +1

Oxidation state of hydrogen on product side: 0

Thus, the oxidation state of hydrogen is changing.

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Oxidation state of hydrogen on reactant side: +1

Oxidation state of hydrogen on product side: +1

Thus, the oxidation state of hydrogen is not changing.

Hence, the correct answer is 2Na(s)+2H_2O(l)\rightarrow 2NaOH(aq.)+H_2(g)

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