All categories

4 years ago

An anode is an electrode immersed in the half-cell where _____ takes place.

Chemistry

2 answers:

siniylev [52]4 years ago

8 0

The electrodes where oxidation occurs during a cell's oxidation-reduction reaction.

MrMuchimi4 years ago

5 0

If I'm not mistaken, the answer should be B. Oxidation

You might be interested in

Give the formula of the conjugate base of each of the following. (Type your answer using the format CO2 for CO2, (NH4)2CO3 for (

MissTica

Answer:

a) [NH2]-,

b) [O]2-

c) [Cl]-

Explanation:

The conjugate base is the base member (X⁻) of a weak acid (HX). In other words, the conjugate base is the remaining substance due to the proton loss in the acid HX.

a) For NH₃, (HX; X: NH₂⁻), conjugate base is NH₂⁻. In the format, [NH2]-.

b) For OH⁻, (HX; X: O²⁻), conjugate base is O²⁻. In the format, [O]2-.

c) For HCl, (HX; X: Cl⁻), conjugate base is Cl⁻. In the format, [Cl]-.

7 0

3 years ago

Hello there!

Alenkasestr [34]

Answer:

Mass of carbon dioxide = 7.48 g

Explanation:

Given data:

Mass of lithium carbonate = 12.5 g

Mass of carbon dioxide produced = ?

Solution:

Chemical equation:

Li₂CO₃ → Li₂O + CO₂

Number of moles of Li₂CO₃:

Number of moles = mass/ molar mass

Number of moles = 12.5 g /73.89 g/mol

Number of moles = 0.17 mol

Now we will compare the moles of Li₂CO₃ with CO₂.

Li₂CO₃ : CO₂

1 : 1

0.17 : 0.17

Mass of carbon dioxide:

Mass of carbon dioxide = number of moles × molar mass

Mass of carbon dioxide = 0.17 mol × 44 g/mol

Mass of carbon dioxide = 7.48 g

4 0

3 years ago

What is potential energy?

Vlad [161]

Answer:

Explanation:

it is the energy stored in the chemical bonds of a substance

4 0

2 years ago

Read 2 more answers

For which of the following species are the dispersion forces strongest?

tigry1 [53]

In order to see which species has the strongest dispersion forces, you need to calculate their molar mass, because the higher the molar mass, the stronger the dispersion forces.
Since E. C8H18 has the highest molar mass, its dispersion forces are also the strongest ones.

5 0

3 years ago

Aqueous sulfuric acid reacts with solid sodium hydroxide to produce aqueous sodium sulfate and liquid water . If of water is pro

sergeinik [125]

The question is incomplete, here is the complete question:

Aqueous sulfuric acid reacts with solid sodium hydroxide to produce aqueous sodium sulfate and liquid water. If 12.5 g of water is produced from the reaction of 72.6 g of sulfuric acid and 77.0 g of sodium hydroxide, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.

Answer: The percent yield of water in the reaction is 46.85 %.

Explanation:

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

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

For NaOH:

Given mass of NaOH = 77.0 g

Molar mass of NaOH = 40 g/mol

Putting values in equation 1, we get:

$\text{Moles of NaOH}=\frac{77.0g}{40g/mol}=1.925mol$

For sulfuric acid:

Given mass of sulfuric acid = 72.6 g

Molar mass of sulfuric acid = 98 g/mol

Putting values in equation 1, we get:

$\text{Moles of sulfuric acid}=\frac{72.6g}{98g/mol}=0.741mol$

The chemical equation for the reaction of NaOH and sulfuric acid follows:

$H_2SO_4+2NaOH\rightarrow Na_2SO_4+2H_2O$

By Stoichiometry of the reaction:

1 mole of sulfuric acid reacts with 2 moles of NaOH

So, 0.741 moles of sulfuric acid will react with = $\frac{2}{1}\times 0.741=1.482mol$ of NaOH

As, given amount of NaOH is more than the required amount. So, it is considered as an excess reagent.

Thus, sulfuric acid is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of sulfuric acid produces 2 moles of water

So, 0.741 moles of sulfuric acid will produce = $\frac{2}{1}\times 0.741=1.482moles$ of water

Now, calculating the mass of water from equation 1, we get:

Molar mass of water = 18 g/mol

Moles of water = 1.482 moles

Putting values in equation 1, we get:

$1.482mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=(1.482mol\times 18g/mol)=26.68g$

To calculate the percentage yield of water, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of water = 12.5 g

Theoretical yield of water = 26.68 g

Putting values in above equation, we get:

$\%\text{ yield of water}=\frac{12.5g}{26.68g}\times 100\\\\\% \text{yield of water}=46.85\%$

Hence, the percent yield of water in the reaction is 46.85 %.

8 0

3 years ago