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3 years ago

Qué tipo de reacción es el siguiente? CH4 + 02 CO2 + H2O

Chemistry

2 answers:

Tatiana [17]3 years ago

7 0

Answer:

Combustion reaction

Explanation:

Let's consider the following balanced equation.

CH₄ + 2 O₂ ⇒ CO₂ + 2 H₂O

This reaction is known as a combustion reaction, in which a compound reacts with oxygen to form a compound of carbon and water.

If the product is carbon dioxide, the combustion is complete.
If the product is carbon monoxide or carbon, the combustion is incomplete.

nignag [31]3 years ago

3 0

Answer:

It is a combustion reaction, where the compound METHANE, which would be CH4, is combusted

Explanation:

In combustion, the reactants are always the compound that will combuste the most oxygen, and in the products there is water and carbon dioxide as the product.

But there are two types of combustions, the complete and the incomplete, in this case how the methane was completely combusted and not in a partial way it would be a complete combustion.

Combustion reactions are EXOTHERMIC AND IRREVERSIBLE reactions.

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An iron ore contains 39% Fe2O3 by mass. What is the maximum mass of iron that can be recovered from 13.2 kg of this ore?

Mars2501 [29]

Answer:

3.6036

Explanation:

0.39 * 13.2 = 5.148

5.148 * 0.7 = 3.6036

Fe2O3 = 0.7

6 0

3 years ago

G(1)=0 g(n) =g(n-1)+n g(2)=

Aliun [14]

G(2)=2

For this, you can plug in 2 everywhere you see an n. So the equation will read:
g(2)=g(2-1)+2 -> g(2)=g(1)+2. Since we are given g(1)=0, we can plug in 0 where we see g(1). The equation is now. g(2)=0+2. So, g(2)=2.

6 0

3 years ago

3) How many micrograms are found in 9.12 x 10-5 L of Water?

Ann [662]

Answer:

86.2 or 431/5

Explanation:

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6 0

3 years ago

A 5.000 g sample of Niso4 H2O decomposed to give 2.755 g of anhydrous NiSO4.

Vinvika [58]

Answer:

a) 7.0.

b) Nickel sulfate hepta hydrate.

c) 280.83 g/mol.

d) 44.9%.

Explanation:

a) What is the formula of the hydrate?

The mass of the hydrated sample (NiSO₄.xH₂O) = 5.0 g,

The mass of the anhydrous salt (NiSO₄) = 2.755 g,

The mass of water = 5.0 g - 2.755 g = 2.245 g.

∴ no. of moles of water = mass/molar mass = (2.245 g)/(18.0 g/mol) = 0.1247 mol.

∴ no. of moles of anhydrous salt (NiSO₄) = mass/molar mass = (2.755 g)/(154.75 g/mol) = 0.0178 mol.

∴ water of crystallization in the sample (x) = no. of moles of water/no. of moles of anhydrous salt (NiSO₄) = (0.1247 mol)/(0.0178 mol) = 7.0.

b) What is the full chemical name for the hydrate?

The name of the salt (NiSO₄.7H₂O) is Nickel sulfate hepta hydrate.

c) What is the molar mass of the hydrate?

(NiSO₄.7H₂O)

The molar mass = molar mass of NiSO₄ + 7(molar mass of H₂O) = (154.75 g/mol) + 7(18.0 g/mol) = 280.83 g/mol.

d) What is the mass % of water in the hydrate?

The mass % of water = (mass of water)/(mass of hydrated sample) x 100 = (2.245 g)/(5.0 g) x 100 = 44.9%.

8 0

3 years ago

6. 7. A hyperbaric chamber has a volume of 200. L. (a) How many moles of oxygen are needed to fill the chamber at room temperatu

Otrada [13]

Answer:

a) 24.7 mol

b) 790 g

Explanation:

Step 1: Given data

Volume of the chamber (V): 200. L

Room temperature (T): 23 °C

Pressure of the gas (P): 3.00 atm

Step 2: Convert "T" to Kelvin

We will use the following expression.

K = °C + 273.15

K = 23°C + 273.15 = 296 K

Step 3: Calculate the moles (n) of oxygen

We will use the ideal gas equation.

P × V = n × R × T

n = P × V/R × T

n = 3.00 atm × 200. L/(0.0821 atm.L/mol.K) × 296 K = 24.7 mol

Step 4: Calculate the mass (m) corresponding to 24.7 moles of oxygen

The molar mass (M) of oxygen ga sis 32.00 g/mol. We will calculate the mass of oxygen using the following expression.

m = n × M

m = 24.7 mol × 32.00 g/mol = 790 g

6 0

3 years ago