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Juli2301 [7.4K]
3 years ago
11

If 80.0 grams of oxygen gas is consumed with a stoichiometric equivalent of aluminum metal, how many grams of aluminum oxide (mo

lar mass = 102 g/mol) would be produced?
Chemistry
1 answer:
Pachacha [2.7K]3 years ago
8 0

Answer:

170 g

Explanation:

Moles of Oxygen gas :

Given, Mass of Oxygen = 80.0 g

Molar mass of Oxygen gas= 31.998 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{80.0\ g}{31.998\ g/mol}

Moles\ of\ O_2=2.5\ mol

The reaction between Al and O₂ is shown below as:

4Al + 3O₂ ⇒ 2Al₂O₃

From the reaction,

3 moles of O₂ on reaction forms 2 moles of Al₂O₃

1 mole of O₂ on reaction forms 2/3 moles of Al₂O₃

2.5 moles of O₂ on reaction forms (2/3)*2.5 moles of Al₂O₃

Moles of Al₂O₃ = 1.6667 moles

Molar mass of Al₂O₃ = 102 g/mol

Mass = Moles * Molar mass = 1.6667 * 102 g = 170 g

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6 0
3 years ago
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The bonds in the reactants of Figure 7-3 contained 372 kJ of chemical energy and the bonds in the products contained 350 kJ of c
satela [25.4K]

Answer: 22 kJ amount of energy is released in the following reaction.

Explanation: There are two types of reaction on the basis of amount of heat absorbed or released.

1. Endothermic reactions: These are the type of reactions in which reactants absorb heat to form the products. The energy of the reactants is less than the energy of the products.

2. Exothermic reactions: These are the type of reactions in which heat is released from the chemical reactions. The energy of the products is less than the reactants.

Sign convention for \Delta H: This value is negative for exothermic reactions and positive for endothermic reactions.

For the given chemical reaction,

Energy of the products is less than the energy of the reactants, Hence, this reaction will be a type of exothermic reaction and energy will be released during this chemical change.

Amount of energy released = (350 - 372) kJ = -22kJ

Negative sign symbolizes the energy is being released. So, 22 kJ amount of energy is released in the following reaction.

6 0
3 years ago
What is the total enthalpy change for the reaction? Is the reaction exothermic or endothermic?
Nuetrik [128]

Answer: S8(s) + 8O2(g) → 8SO2(g) ΔH = -2368 kJ a.

8 0
3 years ago
Yet a third pair of compounds of manganese and oxygen is 50.48% and 36.81% oxygen respectively. In what small whole number ratio
Mariulka [41]

Answer:

The number ratio is 4:7

Explanation:

Step 1: Data given

Compound 1 has 50.48 % oxygen

Compound 2 has 36.81 % oxygen

Molar mass oxygen = 16 g/mol

Molar mass manganese = 54.94 g/mol

Step 2: Calculate % manganes

Compound 1: 100 - 50.48 = 49.52 %

Compound 2: 100 - 36.81 = 63.19 %

Step 3: Calculate mass

Suppose mass of compounds = 100 grams

Compound 1:

 50.48 % O = 50.48 grams

 49.52 % Mn = 49.52 grams

Compound 2:

36.81 % O = 36.81 grams

63.19 % Mn = 63.19 grams

Step 4: Calculate moles

Compound 1

Moles O = 50.48 grams / 16.0 g/mol = 3.155 moles

Moles Mn = 49.52 grams / 54.94 g/mol = 0.9013 moles

Compound 2

Moles O = 36.81 grams / 16.0 g/mol = 2.301 moles

Moles Mn = 63.19 grams / 54.94 g/mol = 1.150 moles

Step 5: calculate mol ratio

We will divide by the smallest amount of moles

Compound 1

O: 3.155/0.9013 = 3.5

Mn: 0.9013 / 0.9013 = 1

Mn2O7

Compound 2

O: 2.301 / 1.150 = 2

Mn: 1.150 / 1.150 = 1

MnO2

The number ratio is 2:3.5 or 4:7

7 0
3 years ago
PLEASE HURRY AND SHOW WORK
IgorC [24]

Answer:

The answer to your question is   P = 1.64 atm

Explanation:

Data

Volume = 2.5 x 10⁷ L

Temperature = 22°C

Pressure = ?

Moles = 1.7 x 10⁶

R = 0.082 atm L/ mol°K

Process

1.- Convert temperature to °K

Temperature = 22 + 273

                      = 295°K

2.- Use the Ideal gas law to solve this problem

                PV = nRT

- Solve for P

                P = nRT / V

- Substitution

                P = (1.7 x 10⁶)(0.082)(295) / 2.5 x 10⁷

- Simplification

                P = 41123000 / 2.5 x 10⁷

- Result

                P = 1.64 atm

3 0
3 years ago
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