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2 years ago

Which is the correct number of moles of NO that is produced from 13.2 moles of oxygen

Chemistry

1 answer:

Oksanka [162]2 years ago

5 0

<h3>Answer:</h3>

10.6 mol NO

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right<u> </u>

<u>Chemistry</u>

<u>Stoichiometry</u>

Using Dimensional Analysis

<h3>Explanation:</h3>

<u>Step 1: Define</u>

[RxN - Balanced] 4NH₃ + 5O₂ → 4NO + 6H₂O

[Given] 13.2 mol O₂

<u>Step 2: Identify Conversions</u>

[RxN] 5 mol O₂ → 4 mol NO

<u>Step 3: Stoich</u>

[DA] Set up: $\displaystyle 13.2 \ mol \ O_2(\frac{4 \ mol \ NO}{5 \ mol \ O_2})$
[DA] Multiply/Divide [Cancel out units]: $\displaystyle 10.56 \ mol \ NO$

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 3 sig figs.</em>

10.56 mol NO ≈ 10.6 mol NO

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If 1.6 moles of an ideal gas are at a temperature of 25c and a pressure of 0.91 atm hg, what volume would the gas occupy, in lit

Fiesta28 [93]

$From\ Ideal\ Gas\ Law:\\\\PV=nRT\\\\
P-pressure\\V-volume\\n-number\ of\ moles\\R- universal\ gas\ constant\\T-absolute\ tmeperature\\\\
R=\ 8,3145J/ mol\ K\\P=0,91atm\\
n=1,6moles\\T=25c\\\\
Converting\ units:\\\\
1atm=101,3kPa=101,3*10^3\\
0,91atm=0,91*101,3*10^3=92,183*10^3Pa\\T=25c=273+25=298K\\\\
V=\frac{nRT}{P}=\frac{1,6*8,3145*298}{92183}=0,043m^3=43liters\\\\Answer\ is\ 43\ liters.$

8 0

3 years ago

The black, granular material that fills a dry cell in a common flashlight (between the carbon rod and the zinc shell) is mangane

mestny [16]

Answer: c. +4

Explanation:

For formation of a neutral ionic compound, the charges on cation and anion must be balanced. The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.

$Mn:25:1s^22s^22p^63s^23p^64s^23d^{5}$

$Mn^{4+}:21:1s^22s^22p^63s^23p^63d^1$

$O:8:1s^22s^22p^4$

$O^{2-}:10:1s^22s^22p^6$

Here manganese is having an oxidation state of +4 called as cation and oxygen forms an anion with oxidation state of -2. Thus they combine and their oxidation states are exchanged to give $Mn_2O_4$ which written in simplest whole number ratios to give neutral $MnO_2$

7 0

3 years ago

What is the oxidation half-reaction for this unbalanced redox equation? cr2o72– + fe2+ → cr3+ + fe3+ cr3+ → cr2o72– cr2o72– → cr

KatRina [158]

Answer:

6Fe^2+(aq) -------> 6Fe^3+(aq) + 6e

Explanation:

The balanced oxidation half equation is;

6Fe^2+(aq) -------> 6Fe^3+(aq) + 6e

A redox reaction is actually an acronym for oxidation-reducation reaction. Since the both reactions are complementary, there can't be oxidation without reduction and there can't be reduction without oxidation.

The main characteristic of redox reactions is that electrons are transferred in the process. The number of electrons transferred is usually deduced from the balanced reaction equation. For this reaction, the balanced overall reaction equation is;

Cr2O7^2–(aq) + 6Fe^2+(aq) +14H^+(aq)→ 2Cr^3+(aq) + 6Fe^3+ (aq) + 7H2O(l)

It is clear from the equation above that six electrons were transferred. Thus six Fe^2+ ions lost one electron each in the oxidation half equation as shown in the balanced oxidation half equation above.

4 0

3 years ago

Which of the substances are elements please help

ivanzaharov [21]

Answer:

Substances 1 and 2

Explanation:

an element only has 1 kind of atoms :3

6 0

3 years ago

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3 years ago

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