All categories

3 years ago

Which type of organic reaction produces both water and carbon dioxide?

2 answers:

6 0

I believe the correct answer from the choices listed above is option 2. The type of organic reaction that produces both water and carbon dioxide would be combustion. It<span> usually occurs when a hydrocarbon reacts with oxygen to produce carbon dioxide and water.</span>

ankoles [38]3 years ago

4 0

the correct answer is combustion

when an organic compounds burns in the presence of oxygen the products are carbon dioxide and water. Combustion reactions yields a large amount of energy

an example for combustion reaction is as follows

combustion of methane;

CH₄ + 2O₂ --> CO₂ + 2H₂O

correct answer is

2. combustion

You might be interested in

Shifts in the rock layer locations cannot account for gaps in the rock record<br><br> true or false

vivado [14]

Answer: That would be false because it is the contact between two layers representing a gap in the geologic record, usually from the erosion of the layers which would normally be expected to appear.

Explanation:

Have a good day

I hope this helps if not sorry :(

Stay motivated

4 0

3 years ago

How many milliliters of 2.00 M H2SO4 will react with 28.0 g of NaOH?

77julia77 [94]

Answer:175⋅mL of the given sulfuric acid

Explanation:

5 0

3 years ago

A 0.5922 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl

Elanso [62]

<u>Answer:</u> The mass percent chlorine in pure chloride compound is 56.31 %.

<u>Explanation:</u>

We are given:

Mass of AgCl precipitated = 1.3487 g

We know that:

Molar mass of AgCl = 143.32 g/mol

Molar mass of Chlorine atom = 35.45 g/mol

As, all the chlorine in the sample is precipitated to silver chloride. So, the mass of chlorine in silver chloride will be equal to the mass of chlorine present in the sample.

To calculate the mass of chlorine in given mass of AgCl, we apply unitary method:

In 143.32 g of silver chloride, mass of chlorine present is 35.45 g

So, in 1.3487 g of silver chloride, mass of chlorine present will be = $\frac{35.45g}{143.32g}\times 1.3487g=0.3335g$

To calculate the percentage composition of chlorine in pure chloride compound, we use the equation:

$\%\text{ composition of chlorine}=\frac{\text{Mass of chlorine}}{\text{Mass of pure chloride compound}}\times 100$

Mass of pure chloride compound = 0.5922 g

Mass of chlorine = 0.3335 g

Putting values in above equation, we get:

$\%\text{ composition of chlorine}=\frac{0.3335g}{0.5922g}\times 100=56.31\%$

Hence, the mass percent chlorine in pure chloride compound is 56.31 %.

6 0

4 years ago

Provide an explanation at the subatomic level to explain why different colors are observed for different metal salts.

lakkis [162]

Answer:

When you heat an atom, some of its electrons are "excited* to higher energy levels. When an electron drops from one level to a lower energy level, it emits a quantum of energy. ... The different mix of energy differences for each atom produces different colours. Each metal gives a characteristic flame emission spectrum.

Explanation:

8 0

4 years ago

Read 2 more answers

Nearly every compound of silicon has the element in the ⁺4 oxidation state. In contrast, most compounds of lead have the element

baherus [9]

Boron shows analogous behaviour with silicon. Every compound of Boron have +3 oxidation state, while as we go down the the oxidation state become +1 and +3. For example, gallium, indium, etc.

Similarly, every compound of silicon has the element in the ⁺4 oxidation state. In contrast, most compounds of lead have the element in the ⁺2 state because of inert pair effect.

<h3>What is Inert pair effect? </h3>

The inert-pair effect is defined as the tendency of two electrons in the outermost atomic s-orbital almost remain unshared in the compounds of the post-transition metals.

<h3>How we calculate Oxidation state? </h3>

Each atom in an element either be in its uncombined or free state has oxidation number of zero. Such as each atom in H₂, Cl₂ , P4, ,O₂ , Na, Al, O3, S8, and Mg, all have an oxidation number zero.
The oxidation state of ions that comprise of only one atom is the actual charge on the ion.
The oxidation state of hydrogen is +1, excluding when it is bonded to metals having two elements. For example, CaH2, its oxidation state is –1.
Fluorine and other halogens have an oxidation state equal to –1 when they appear as a form of halide ions in their compounds.

Since the inert pair effect increases as we go down the group and become more predominant, therefore, the stability of +2 oxidation state goes on increasing down the group. Therefore, gallium, indium are mostly found in +1 oxidation state.

Thus, we concluded that Boron shows analogous behaviour with silicon. Every compound of Boron have +3 oxidation state, while as we go down the the oxidation state become +1 and +3. For example, gallium, indium, etc.

learn more about oxidation state:

brainly.com/question/25551544

#SPJ4

4 0

2 years ago