Using P1V1/T1 = P2V2/T2, 1 being the conditions initially and 2 being the secondary conditions…. always make sure you convert you units first , L=695.8262L

8 0

3 years ago

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

Oksanka [162]

<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

5 0

3 years ago

Calculate the number of photons having a wavelength of 12.0 μm required to produce 1.0 kJ of energy.

nika2105 [10]

Answer:

N = 603.32 × 10 ²⁰

Explanation:

Given data:

Wavelength of photon = 12.0 μm or 12 × 10 ⁻⁶ m

Energy = 1.0 KJ or 1000 j

Number of photons = ?

Solution:

Formula:

E = n . h . f

E = energy

N = number of photons

h = planck's constant

f = frequency

it is known that

f = c/λ

thus,

E = N . h . c / λ

Now we will put the values in formula.

1000 j = ( N. 6.63 × 10 ⁻³⁴ j.s × 3 × 10⁸ m/s ) / 12 × 10 ⁻⁶ m

N = 1000 j ×12 × 10 ⁻⁶ m / 6.63 × 10 ⁻³⁴ j.s × 3 × 10⁸ m/s

N = 12000 j × 10 ⁻⁶ m / 19.89 × 10 ⁻²⁶ j. m

N = 603.32 × 10 ²⁰

4 0

3 years ago

How many degrees does the earth tilt

mart [117]

That would be 23.5 degrees

6 0

3 years ago

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