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3 years ago

When the equation Fe + Cl2 ----> FeCl3 is correctly balanced the coefficient for Cl2 is

1 answer:

4 0

The correct answer is D. Using the law of conservation of mass the number of atoms on each side of the equation should be equal. Through introspection, we find that there are 2 $Cl$ atoms on reactant side as opposed 3Cl atoms on product side. If we add a coefficient of 3 on $Cl_2$ we get

$Fe + 3Cl_2 ==> FeCl_3$ .

Now there are 6Cl atoms on reactant side and 2 on product side, hence we add a coefficient of 2 on both $FeCl_3$ and $Fe$ . The balanced chemical equation is,

$2Fe + 3Cl_2 ==> 2FeCl_3$

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A typical aspirin tablet contains 327 mg of acetylsalicylic acid, HC9H7O4. Calculate the pH of a solution that is prepared by di

yawa3891 [41]

Answer:

2.8

Explanation:

First, we will calculate the molarity of the acetylsalicylic acid solution.

M = mass of solute (g) / molar mass of solute × volume of solution (L)

M = 0.327 g / 180.158 g/mol × 0.237 L

M = 7.66 × 10⁻³ M

For a weak acid such as acetylsalicylic acid, we can find the concentration of H⁺ using the following expression.

[H⁺] = √(Ca × Ka)

where,

Ca: concentration of the acid

Ka: acid dissociation constant

[H⁺] = √(7.66 × 10⁻³ × 3.3 × 10⁻⁴)

[H⁺] = 1.6 × 10⁻³ M

The pH is:

pH = -log [H⁺]

pH = -log 1.6 × 10⁻³ = 2.8

6 0

3 years ago

Two atoms that share one electron each between have a ?

evablogger [386]

Answer:

Covalent bond

Explanation:

A covalent bond is defined as the sharing of election pairs between atoms

8 0

2 years ago

Mrs tuckers class is doing an experiment they fill up a cup with ice water they measure the temperature of both the water and th

ELEN [110]

C.

Hope this is the correct answer

8 0

2 years ago

What happens to the solar energy absorbed by plants during photosynthesis ?

zzz [600]

Answer:

Photosynthesis in plants converts solar energy into chemical energy using electrons and protons from water. in plants involves a series of steps and reactions that use solar energy, water, and carbon dioxide to produce organic compounds and oxygen.

Explanation:

7 0

2 years ago

Read 2 more answers

A 13.30 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 13.00 grams of CO2 and 2

a_sh-v [17]

Answer: The empirical and molecular formula for the given organic compound is $CHO_2$ and $C_2H_2O_4$

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of $CO_2=13.00g$

Mass of $H_2O=2.662g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 13.00 g of carbon dioxide, $\frac{12}{44}\times 13.00=3.54g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 2.662 g of water, $\frac{2}{18}\times 2.662=0.296g$ of hydrogen will be contained.

Mass of oxygen in the compound = (13.30) - (3.54 + 0.296) = 9.464 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{3.54g}{12g/mole}=0.295moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.296g}{1g/mole}=0.296moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{9.465g}{16g/mole}=0.603moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.295 moles.

For Carbon = $\frac{0.295}{0.295}=1$

For Hydrogen = $\frac{0.296}{0.295}=1$

For Oxygen = $\frac{0.603}{0.295}=2.044\approx 2$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 1 : 1 : 2

Hence, the empirical formula for the given compound is $CHO_2$

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is :

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

We are given:

Mass of molecular formula = 90.04 g/mol

Mass of empirical formula = 45 g/mol

Putting values in above equation, we get:

$n=\frac{90.04g/mol}{45g/mol}=2$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_{(1\times 2)}H_{(1\times 2)}O_{(2\times 2)}=C_2H_2O_4$

Hence, the empirical and molecular formula for the given organic compound is $CHO_2$ and $C_2H_2O_4$

3 0

3 years ago