The combustion of glucose is represented by the following balanced equation:

Answer:

C) 4Fe + 3O2 → 2Fe2O3

Explanation:

For this question, first you would go through all the options and make sure that there is an equal amount of elements on each side.

For the first option: 2Fe +02 → 2Fe2O3

You have only 2Fe atoms and 2O atoms on your reactant side and 4Fe and 6O atoms on your product side. This is not balanced.

For option b: 3Fe +302 → 3Fe2O3

You have 3Fe and 6O atoms on your reactant side while on your product side you have 6Fe and 6O atoms. This is not balanced.

For option c: 4Fe +302 → 2Fe2O3

You have 4Fe and 6O atoms on your reactant side and 4Fe and 6O atoms on your product side. This is balanced!

For option d: Fe +0₂ → Fe₂O3

You have 1Fe and 2O atoms on your reactant side and 2Fe and 3O atoms on your product side. This is not balanced.

***Remember to multiply the subscript of an element by their coefficient (number in front of molecule) if there is any.

Answer

Explanation

Given:

Mass composition: 3.758 g carbon, 0.316 g hydrogen, and 1.251 grams oxygen.

What to find:

The empirical formula for the substance.

Step-by-step solution:

The first step is to convert the number of grams of each element into moles as shown below using the molar masses of H = 1.00784 g/mol and C = 12.011 g/mol and O = 15.999 g/mol

Note: Mole = Mass/Molar mass

Moles C = 3.758g/12.011 g/mol = 0.31 mol

Moles H = 0.316g/1.00784 g/mol = 0.31 mol

Moles O = 1.251g/15.999 g/mol = 0.078 mol

Now, let's divide the number of moles of each element by the smallest number obtained:

C = 0.31/0.078 = 4

H = 0.31/0.078 = 4

O = 0.078/0.078 = 1

The empirical formula for the compound is C₄H₄O₁

Dalton's Law or Law of Partial Pressures says that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas that composes it. The partial pressure of a gas on the other hand is defined as the pressure it would exert if it were alone in the container.

So we need to sum all the values:

64 + 50.8 = 114.8 kPa

Answer: 114.8 kPa

Color of reactant. Option B is correct

This is defined as the speed at which a reaction takes place. It can be expressed in terms of the concentration of reactants or products formed per unit time.

The following are the factors that affects reaction rate.

- concentration of a reactant

- Temperature

- Nature of the reactant

- Surface Area

- Catalysts.

Based on the explanations above, we can conclude that the color of reactant will not affect the rate of a reaction

Answer:

5.546262 x 10^24 formula units

Explanation:

Use avogadro's number

9.21 mol CaO ((6.022 x 10^23 formula units CaO)/1 mol CaO)) = 5.546 x 10^24.

I rounded to 3 sig figs.

Answer:

48 minutes

Explanation:

60 divided by 25 equals 2.4 then you times 2.4 by 20

Answer:

D- Br

Explanation:

In this question, we have to find the number of atoms in 12.5 moles of Sulfur, and the way to do it is by using the Avogadro's number, which is 6.02*10^23 atoms, this value represents how many atoms we have in 1 single mol of any element. Therefore in 12.5 moles we will have:

1 mol = 6.02*10^23 atoms

12.5 moles = x atoms

x = 7.52*10^24 atoms of Sulfur in 12.5 moles

When salt dissolves in water, dissociation occurs. This dissociation forms two ions, one positive and one negative. Water is polar and its molecules has poles negatives and positives. So positive poles of water will surround the negative ions. While negative poles will surround the positive ions.

Answer: Alternative "B"

The volume of the cylinder filled with 23.0 g of N₂ gas at a temperature of 65 °C and a pressure of 2.37 atm is 9.6 L

Given that,

Mass of the nitrogen gas in the cylinder (m) = 23 g

Temperature (T) = 65 ℃ = 65 + 273 = 338 K

Pressure (P) = 2.37 atm

R (gas constant) = 0.082057338 L.atm.K⁻¹.mol⁻¹

In Ideal gas law or general gas equation,

PV = nRT

Number of moles in nitrogen (n) = Given mass (m) of nitrogen/ Molar mass of nitrogen

Given mass (m) = 23 g

Molar mass of Nitrogen = 28 g/mol

Number of moles of nitrogen (n) = 23 / 28 = 0.82 moles of nitrogen

PV = nRT

2.37 * V = 0.82 * 0.0821 * 338

2.37 * V = 22.75

V = 22.75 / 2.37

V = 9.6 L

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Answer:

Explanation:

Answer to the 1st one. I have my doubts for the second one so didn't post :)

The empirical formula for a compound composed of 9.93% carbon, 58.6% chlorine, and 31.4% fluorine is CCl₂F₂.

To write the empirical formula, let us assume that total mass of the compound is 100 g, then-

Mass of carbon = 9.93 g

Mass of chlorine = 58.6 g

Mass of fluorine = 31.4 g

We know that,

Molar mass of Carbon = 12.0 g/mol

Molar mass of Chlorine = 35.5 g/mol

Molar mass of Fluorine = 18.9 g/mol

Now, we will calculate the number of moles of each using the formula -

Number of moles = Given mass

                                 Molar mass

Moles of Carbon =   9.93 g     = 0.82 mol

                               12.01 g/mol

Moles of Chlorine =    58.6 g     = 1.65 mol

                                 35.5 g/mol

Moles of fluorine =    31.4 g     = 1.66 mol

                                18.9 g/mol

Now, divide each value with the smallest amount of mole we got,

carbon = 0.82 = 1

               0.82

chlorine = 1.65 =  2

                 0.82

fluorine = 1.66 = 2

                0.82

Therefore, the empirical formula of the compound can be written as - CCl₂F₂

To learn more about empirical formula,

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First, we assume STP conditions and Ideal gas conditions.

In STP conditions, we say that:

1 mol of any gas = 22.4 L (liters)

Procedure:

1 mol Xe ------ 22.4 L (STP)

4.51 moles Xe ------- X

X = 101 L

Answer: 101 L