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2 years ago

Predict the product(s) and write a balanced equation for each of the following redox reactions:

1 answer:

3 0

The balanced equation for when pentane gas (C5H12) combusts with oxygen gas (O2) to form water (H2O) and carbon dioxide (CO2) is

All redox reactions can be divided into two categories: reduction reactions and oxidation reactions. The oxidation-reduction reaction, commonly referred to as the redox reaction, always comprises concurrent oxidation and reduction reactions.

<h3>What results from the simplest interaction between oxygen and pentane?</h3>

The most fundamental oxygen-pentane reaction is combustion. Along with producing water and carbon dioxide, combustion also produces a lot of heat.

<h3>When pentane is burned, what happens?</h3>

In addition, this process generates a lot of heat and light, which we interpret as fire. In the absence of sufficient oxygen for a full combustion, pentane produces carbon monoxide (CO) rather than dioxide (CO2). Never burn any fuel inside a building, not even pentane!

<h3>What is the chemical equation for burning pentane?</h3>

C5H12 is pentane. It produces 5 carbon dioxide and 6 water when fully burned. 8 O2 + C5H12 = 5 CO2 + 6 H2O. This process also produces a great deal of heat and light, which we perceive as fire.

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What is the molecular weight, density, and how many moles in

OverLord2011 [107]

Answer:

<em>1) Molecular weight: 18g/mol </em>

<em>Density: at room temperature (25ºC) is 0.997g/mL</em>

<em>Moles: 0.55moles</em>

<em>2) Molecular weight: 182g/mol</em>

<em>Density: at room temperature (25ºC) is 1.11g/mL</em>

<em>Moles: $2.2x10^{-4}moles$ </em>

Explanation:

1) The molecular formula of water is $H_{2}O$ thus, the molecular weight is the sum of the weights of its atoms.

H: 1g/mol x 2 = 2g/mol

O: 16g/mol x 1 = 16g/mol

$H_{2}O$ : 2g/mol + 16g/mol = 18g/mol

The density (δ) of water at room temperature (25ºC) is 0.997g/mL

Therefore, the weight (m) of 1mL of water is:

m = δ.V = $0.997\frac{g}{mL}. 1mL = 0.997g$

Multiplying the mass by its molecular weight gives the number of moles:

$\frac{0.997g }{18g/mol} = 0.55 moles$

2) The molecular formula of benzophenone is $C_{13}H_{10}O$ thus, the molecular weight is the sum of the weights of its atoms.

C: 12g/mol x 13 = 156g/mol

H: 1g/mol x 10 = 10g/mol

O: 16g/mol x 1 = 16g/mol

$C_{13}H_{10}O$ : 156g/mol + 10g/mol + 16g/mol = 182g/mol

The density (δ) of water at room temperature (25ºC) is 1.11g/mL

Multiplying the mass by its molecular weight gives the number of moles:

$\frac{0.04g }{182g/mol} = 2.2x10^{-4}moles$

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4 years ago

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7. Which of the following would lower the pitch of a string instrument's sound?

vfiekz [6]

The correct option is C.

The pitch of a string refers to the quality of sound that is produced by the string when it vibrates. There are three basic factors that affect the quality of pitch of a string, these are: the tension, the thickness of the string and the length of the string. The higher the thickness of the string, the lower the pitch of the string, thus, increasing the thickness of the string will lower the pitch.

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4 years ago

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In the chemical laboratory, why do scientists use a mortar and pestle?

Butoxors [25]

Answer:

B. To decrease surface area of a solute

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3 years ago

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5. In an oxyacetylene welding torch, acetylene (C2H2) burns in pure oxygen with a very hot flame. The reaction is: 2 C2H2 + 5 O2

gulaghasi [49]

11.375 g ethylene is consumed if 35.0 grams of oxygen is allowed to react and 7.875 ml of water will be produced when the 35.0 grams of oxygen is allowed to react.

<h3>What are moles?</h3>

A mole is defined as 6.02214076 × $10^{23}$ of some chemical unit, be it atoms, molecules, ions, or others. The mole is a convenient unit to use because of the great number of atoms, molecules, or others in any substance.

According to the chemical equation for the combustion of ethylene, 5

moles of oxygen are required to react with 2 moles of ethylene, hence

$m_{_C_2_H_2}$ $= 35gX \frac{1 mol}{(2 \;X\; 16)g } X \frac{2 mol}{(5\;mol )} X \frac{26g}{1 mol }$

$m_{_C_2_H_2} = 11.375 g$

Similarly, 5 moles of oxygen are required as a reactant to produce 2 moles of water, thus

$m_{_H_2_O} = 35gX \frac{1 mol}{(2 \;X\; 16)g } X \frac{2 mol}{(5\;mol )} X \frac{18g}{1 mol }$

$m_{_H_2_O} = 7.875 g$

Given that the density of water is $1.0g ml^{-1}$ , therefore

$Density = \frac{Mass \;of \;water}{Volume \;of \;water}$

$Volume \;of \;water = \frac{7.875}{1.0 g ml^{-1}}$

The volume of water = 7.875 ml

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2 years ago

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Calculate the density in g/l of co2 gas at 27 Celsius and 0.500 atm pressure

lesya692 [45]

Answer:

The density of CO₂ gas at 27 Celsius and 0.500 atm is 0.89 $\frac{grams}{L}$

Explanation:

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

<u><em>P*V = n*R*T Equation (A)</em></u>

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas.

Density allows you to measure the amount of mass in a given volume of a substance. So density is defined as the quotient between the mass of a body and the volume it occupies:

$density=\frac{mass}{volume}$