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2 years ago

How many grams of oxygen are required to produce

Chemistry

1 answer:

Likurg_2 [28]2 years ago

8 0

Answer:

8 GRAMS OF OXYGEN WILL BE REQUIRED TO PRODUCE 9 GRAMS OF WATER MOLECULES.

Explanation:

The equation for the reaction is;

2 H + O2 ----> 2 H2O

(H = 1, O = 16)

From the reaction, it can be observed that 1 mole of O2 reacts to form 2 moles of H2O

At STP, using the molar masses of the elememts and compound in the reaction, 32 g of O2 will reacts to form 36 g (18 * 2 g) of H2O

32 g of O2 = 36 g OF H2O

if 9 grams of H2O is produced, the mass of oxygen required to produce it will be:

( 32 * 9 / 36 ) g of O2

= (288 / 36) g

= 8 g of O2

So, 8 grams of Oxygen will be required to produce 9 grams of water.

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A compound's properties are different than the properties of the elements that make it up.

yan [13]

The answer is True because elements in a compound combine and become an entirely different substance with its own unique properties.

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2 years ago

Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel ro

melamori03 [73]

Answer: The mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For nickel:

Given mass of nickel = 14.8 g

Molar mass of nickel = 58.7 g/mol

Putting values in equation 1, we get:

$\text{Moles of nickel}=\frac{14.8g}{58.7g/mol}=0.252mol$

For the given chemical reaction:

$3NiO(s)+2Al(s)\rightarrow 3Ni(l)+Al_2O_3(s)$

For nickel (II) oxide:

By Stoichiometry of the reaction:

3 moles of nickel are produced from 3 moles of nickel (II) oxide

So, 0.252 moles of nickel will be produced from $\frac{3}{3}\times 0.252=0.252mol$ of nickel (II) oxide

Now, calculating the mass of nickel (II) oxide by using equation 1:

Molar mass of nickel (II) oxide = 74.7 g/mol

Moles of nickel (II) oxide = 0.252 moles

Putting values in equation 1, we get:

$0.252mol=\frac{\text{Mass of nickel (II) oxide}}{74.7g/mol}\\\\\text{Mass of nickel (II) oxide}=(0.252mol\times 74.7g/mol)=18.8g$

For aluminium:

By Stoichiometry of the reaction:

3 moles of nickel are produced from 2 moles of aluminium

So, 0.252 moles of nickel will be produced from $\frac{2}{3}\times 0.252=0.168mol$ of aluminium

Now, calculating the mass of aluminium by using equation 1:

Molar mass of aluminium = 27 g/mol

Moles of aluminium = 0.168 moles

Putting values in equation 1, we get:

$0.168mol=\frac{\text{Mass of aluminium}}{27g/mol}\\\\\text{Mass of aluminium}=(0.168mol\times 27g/mol)=4.54g$

Hence, the mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.

4 0

2 years ago

After a 4.626g sample of silver oxide is heated, 4.306g of silver metal remains. What is the empirical formula of the compound?

saw5 [17]

Answer:

The empirical formula is Ag2O.

The empirical formula is Ag2O.Explanation:

The empirical formula is Ag2O.Explanation:The empirical formula is the simplest whole-number ratio of atoms in a compound.

The empirical formula is Ag2O.Explanation:The empirical formula is the simplest whole-number ratio of atoms in a compound.The ratio of atoms is the same as the ratio of moles. So our job is to calculate the molar ratio of Ag to 2O.

do the steps ...

To get this into an integer ratio, we divide both numbers by the smaller value.

From this point on, I like to summarize the calculations in a table.

ElementAgMass/gXMolesXllRatiomllIntegers

—————————————————−———mAgXXXm7.96Xm0.07377Xll2.00mmm2

mlOXXXXl0.59mm0.0369Xml1mmmml1

There are 2 mol of Ag for 1 mol of O.

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Answer:

Explanation:

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Alenkinab [10]

The answer to your question is mayonnaise is colloids.

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3 years ago

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