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3 years ago

6

For below checmical equation (which may or may not be balanced), list the number of each type of atom on each side of the equati

on, and determine if the equation is balanced.
2 C6H14(l) + 19 O2(g) -------> 12 CO2(g) + 14 H2O(g)

1 answer:

Olegator [25]3 years ago

5 0

Answer:

Left hand side:-

Carbon - 12

HYdrogen - 28

Oxygen - 38

Right hand side:-

Carbon - 12

Hydrogen - 28

Oxygen - 38

Since, the number of atoms each side are equal, the reaction is balanced.

Explanation:

The given reaction is:-

$2C_6H_{14}_{(l)}+19O_2_{(g)}\rightarrow 12CO_2_{(g)}+14H_2O_{(g)}$

Left hand side:-

Carbon - 12

HYdrogen - 28

Oxygen - 38

Right hand side:-

Carbon - 12

Hydrogen - 28

Oxygen - 38

<u>Since, the number of atoms each side are equal, the reaction is balanced.</u>

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What do you mean by the circular path that an electron revolves round the nuculeus in an atom?

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Answer:

The circular path and electron revolves around the nucleus in an atom is called shell or orbit.

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3 years ago

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Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water. The equation for the reac

monitta

Answer:

75.5 g O₂ (g) can be produced from 42.6 g of H₂O (g)

Explanation:

<u>1) Balanced chemical equation (given):</u>

2H₂O(g) → 2H₂(g) + O₂(g)

<u>2) Mole ratios:</u>

2 moles H₂O(g) : 2 moles H₂(g) : 2 moles O₂(g)

<u>3) Calculate the number of moles of reactant (H₂0):</u>

number of moles = mass in grams / molar mass

molar mass of water: 18.015 g/mol

mass in grams of water: 42.6 g

number of moles = 42.6 g / 18.05 g/mol = 2.36 moles H₂O

<u>4) Set a proportion using the mole ratio O₂ to H₂O and the actual number of moles of H₂O:</u>

2 moles O₂ / 2 moles H₂O = x / 2.36 moles H₂O

x = 2.36 moles O₂

<u>5) Convert 2.36 moles O₂ to grams:</u>

mass in grams = number of moles × molar mass

mass = 2.36 moles × 32.00 g/mol = 75.5 g O₂

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4 years ago

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Ultraviolet radiation and radiation of shorter wavelengths can damage biological molecules because they carry enough energy to b

DIA [1.3K]

<h3>Answer:</h3>

Longest wavelength = 343.7 nm

<h3>Solution and Explanation:</h3>

In this question we need to first use the concept of energy of a photon.

Energy of a photon, E, is given by the formula, E = hf, where h is the plank's constant, f is the frequency.

But since, f is given by dividing speed, c, by wavelength, λ, then;

E = hc/λ

We are given 348 kJ/mol required to break carbon-carbon bonds.

We know that; 1 mole of bonds = 6.022 × 10^23 bonds.

We are required to find the longest wavelength with enough energy to break the C-C bonds.

This can be worked out in simple steps:

Step 1: Energy required to break one bond (kJ/bond)

1 mole of bonds = 6.022 × 10^23 bonds.

Therefore;

348 kJ = 6.022 × 10^23 bonds.

Thus;

1 bond = 348 kJ ÷ 6.022 × 10^23 bonds.

= 5.778 x 10^-22 kJ

But; 1000 joules = 1 kJ

Hence; energy per bond = 5.778 x 10^-19 Joules

Step 2: Energy per photon

Breaking one bond requires energy equivalent to energy of a photon.

Therefore;

1 photon = 5.778 x 10^-19 Joules

= 5.778 x 10^-19 J/photon

Step 3: Calculating the wavelength

From the equation of energy of a photon;

E = hc/λ

h is the plank's constant = 6.626 × 10^-34 J/s

c is the speed of light in vacuum = 2.9998 × 10^8 m/s

E is the energy of a photon = 5.778 x 10^-19 Joules

Therefore, making λ (wavelength) the subject;

$wavelength = \frac{hc}{E}$

$= \frac{(6.626 . 10^{-34})(92.9998.10^8) }{(5.778 .10^{-19} )}$

$= 3.437. 10^{-7} m$

= 3.437 x 10^-7 m

But; 1 nm = 10^-9 m

Thus;

wavelength = 343.7 nm

Therefore, the longest wavelength of the radiation will be 343.7 nm

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3 years ago

What is a possible quantum number set for an electron in the 3s orbital of a magnesium atom

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<em>n</em> = 3
<em>l</em> = 0
$m_l$ = 0

$m_s$ = 1/2 or -1/2

<h3>Explanation</h3>

There are four quantum numbers in an electron that orbits the atom.

<em>n</em>, the principal quantum number.
<em>l</em>, the angular quantum number.
$m_l$ , the magnetic quantum number.
$m_s$ , the spin quantum number.

<em>n</em> is a positive integer. The value of n indicates the main shell of the electron. The electron in question is in the 3s orbital. As a result, <em>n</em> = 3.

<em>l</em> is a non-negative integer. The value of <em>l</em> indicates the type of subshell ("orbital") of the electron. The types of subshells possible depends on the main shell. For example, both s and p orbitals exist in the second main shell. However, only the s orbital exists in the first main shell. The value of <em>l</em> ranges from 0 to <em>n</em> - 1.

<em>l</em> = 0 indicates an <em>s</em> orbital.
<em>l</em> = 1 indicates a <em>p</em> orbital.
<em>l</em> = 2 indicates a <em>d</em> orbital.
<em>l</em> = 3 indicates an <em>f</em> orbital.

The electron in question is in an <em>s</em> orbital. As a result, <em>l </em>= 0.

$m_l$ is an integer. The value of $m_l$ indicates the position of the electron within the subshell. The range of $m_l$ depends on the value of <em>l</em>. $m_l$ ranges from -<em>l</em> to <em>l </em>(that's <em>-l</em>, ..., -1, 0, 1, ... <em>l</em>). Accordingly, there are 2 <em>l</em> + 1 orbitals in a <em>l</em> subshell. <em>l </em>= 0 for this 3s<em> </em>electron. There's only one orbital in the 3s subshell. The only $m_l$ value possible for this electron is 0.

The value of $m_s$ is either - 1/2 or 1/2. It indicates the position of an electron within a single orbital. The value of $m_s$ does not depend on that of <em>n</em>, <em>l</em>, or $m_l$ . However, by the Pauli Exclusion Principle, at least one of the four numbers must differ for two electrons in the same atom. In case all three of <em>n</em>, <em>l</em>, and $m_l$ are the same, the two electrons must differ in $m_s$ . However, this question asks only for the number of one single electron. Thus, giving either - 1/2 or 1/2 shall work.

<h3>Reference</h3>

Vitz et. al, "5.8 Quantum Numbers (Electronic)", <em>ChemPRIME (Moore et al.)</em>, Chemistry Libretexts. 27 Oct 2017.

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