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3 years ago

What is the definition of electrical energy?

1 answer:

7 0

Answer: Electrical energy is defined as an electric charge that lets work be accomplished. An example of electrical energy is power from a plug outlet. YourDictionary definition and usage example.

Explanation:

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What is the mass of 5.84 × 10^21 atoms of xenon?

podryga [215]

Answer:

5.84e+21

Explanation:

8 0

3 years ago

29.0g silver combine completely with 4.30g of sulfur to form a compound. what is the percent composition of this compound?

Deffense [45]

Answer:

Percentage of silver and sulphur in the compound is 87.08% and 12.91% respectively

Explanation:

Given:

Amount of silver = 29.0 g

Amount of sulphur= 4.30 g

To find:

Percent composition of the compound=?

Solution:

$\text { percent of compound }=\frac{\text { amount of element }}{\text { Total Molecule Mass }} \times 100$

Total Molecule mass = amount of silver + amount of sulphur

Total Molecule mass = 29+4.3

Total Molecule mass = 33.3g

Percentage of silver:

$\text { Percentage of silver }=\frac{\text { amount of silver }}{\text { Total Molecule Mass }} \times 100$

=> $\frac{29.0}{33.3}\times100$

=> $0.8708 \times100$

=> 87.08%

Percentage of silver:

$\text { Percentage of silver }=\frac{\text {amount of suplhur}}{\text { Total Molecule Mass }} \times 100$

=> $\frac{4.30}{33.3}\times 100$

=> $0.1291\times 100$

=> 12.91%

3 0

4 years ago

A 1.00 kg sample of Sb2S3 (s) and a 10.0 g sample of H2 (g) are allowed to react in a 25.0 L container at 713 K. At equilibrium,

Scorpion4ik [409]

Answer: The value of $K_c$ is coming out to be 0.412

Explanation:

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

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

For $Sb_2S_3$

Given mass of $Sb_2S_3$ = 1.00 kg = 1000 g (Conversion factor: 1 kg = 1000 g)

Molar mass of $Sb_2S_3$ = 339.7 g/mol

Putting values in equation 1, we get:

$\text{Moles of }Sb_2S_3=\frac{1000g}{339.7g/mol}=2.944mol$

For hydrogen gas:

Given mass of hydrogen gas = 10.0 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1, we get:

$\text{Moles of hydrogen gas}=\frac{10.0g}{2g/mol}=5mol$

For hydrogen sulfide:

Given mass of hydrogen sulfide = 72.6 g

Molar mass of hydrogen sulfide = 34 g/mol

Putting values in equation 1, we get:

$\text{Moles of hydrogen sulfide}=\frac{72.6g}{34g/mol}=2.135mol$

The chemical equation for the reaction of antimony sulfide and hydrogen gas follows:

$Sb_2S_3(s)+3H_2(g)\rightarrow 2Sb(s)+3H_2S(g)$

Initial: 2.944 5

At eqllm: 2.944-x 5-3x 2x 3x

We are given:

Equilibrium moles of hydrogen sulfide = 2.135 moles

Calculating for 'x', we get:

$\Rightarrow 3x=2.135\\\\\Rightarrow x=\frac{2.135}{3}=0.712$

Equilibrium moles of hydrogen gas = (5 - 3x) = (5 - 3(0.712)) = 2.868 moles

Volume of the container = 25.0 L

Molarity of a solution is calculated by using the formula:

$\text{Molarity}=\frac{\text{Moles}}{\text{Volume}}$

The expression of $K_c$ for above equation, we get:

$K_c=\frac{[H_2S]^3}{[H_2]^3}$

The concentration of solids and liquids are not taken in the expression of equilibrium constant.

$K_c=\frac{(\frac{2.135}{25})^3}{(\frac{2.868}{25})^3}\\\\K_c=0.412$

Hence, the value of $K_c$ is coming out to be 0.412

3 0

3 years ago

The burning of 48.7 g of zns in the presence of oxygen gives 220.0 kj of heat. what is h for the reaction as written below?

mr_godi [17]

Answer : The $\Delta H_{rxn}$ for the reaction is, 54.89 KJ

Solution : Given,

Mass of ZnS = 48.7 g

Molar mass of ZnS = 97.474 g/mole

$\Delta H=220KJ$

First we have to calculate the moles of ZnS.

$\text{ Moles of ZnS}=\frac{\text{ Mass of ZnS}}{\text{ Molar mass of ZnS}}=\frac{48.7g}{97.474g/mole}=0.499moles$

The balanced combustion reaction is,

$2ZnS+3O_2\rightarrow 2ZnO+2SO_2$

From the given reaction, we conclude that

As, 2 moles of ZnS gives energy = 220 KJ

So, 0.499 moles of ZnS gives energy = $\frac{220KJ}{2moles}\times 0.499moles=54.89KJ$

Therefore, the $\Delta H_{rxn}$ for the reaction is, 54.89 KJ

4 0

3 years ago

Read 2 more answers

Calculate the mass of silver chloride required to plate 195 mg of pure silver.

Flura [38]

Given information:

Mass of pure silver = 195 mg

To determine :

Mass of silver chloride required to plate 195 mg of pure silver

Calculation:

The silver chloride used for silver plating usually contains 75.27 % silver

i.e.

every 100 mg of silver chloride will contain 75.27 mg silver

therefore, amount of silver chloride corresponding to 195 mg of silver would be = 195 mg * 100 mg/75.27 mg

= 259.1 mg

7 0

3 years ago