Determine the mass/mass % of 4.0 g of KOH in 50.0 g of solution

Answer:

10.5 L of O₂.

Explanation:

We'll begin by calculating the number of mole in 90 g of C₂H₆. This can be obtained as follow:

Molar mass of C₂H₆ = (12×2) + (6×1)

= 24 + 6

= 30 g/mol

Mass of C₂H₆ = 90 g

Mole of C₂H₆ =?

Mole = mass / molar mass

Mole of C₂H₆ = 90 / 30

Mole of C₂H₆ = 3 moles.

Finally, we shall determine the volume of O₂ required. This is illustrated:

2C₂H₆ + 7O₂ —> 4CO₂ + 6H₂O

From the balanced equation above, we can say that:

2 L of C₂H₆ required 7 L of O₂.

Therefore, 3 L of C₂H₆ will require

= (3 × 7)/ 2 = 10.5 L of O₂.

Thus, 10.5 L of O₂ is required for the reaction.

Answer:

28.466256

Explanation:

Answer:

the answer is something  

Explanation:

Answer:

The answer is gravity and friction.

Explanation:

Answer:

solution given:

log k=4-[tex] \frac{200}{t} [/tex]

so,

On comparison

∆S°/R = 4

∆ S° = 4R

mousam brother is correct

hope it helps you have a good day

Answer:

29.5 days

Explanation:

orginally 27.3 days but 29.5 days is also correct

Answer:

for skin cancer use sunscreen but for cancer that's most common eat healthy and take vitamins as much as you can.

Explanation:

Answer:

3.92%

Explanation:

The solution that is formed is of KCl in water. This means that the percent composition by mass is given by the formula:

We now calculate the mass of solution:

Finally we calculate the percent composition:

The temperature of a gas sample rises, the molecules quicken, and as a result, the root mean square molecular speed rises.

Degree of warmth or coolness determined by a specific scale

The temperature of a gas sample rises, the molecules quicken, and as a result, the root mean square molecular speed rises.

In a gas, the speed of the molecules is inversely related to the molar mass of the gas and inversely proportional to temperature.

The rate of diffusion is inversely related to the square root of the gas's molar mass, according Graham's law of Diffusion.

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Answer:

412 g Cl₂

General Formulas and Concepts:

Atomic Structure

Stoichiometry

Explanation:

Step 1: Define

[Given] 3.50 × 10²⁴ molecules Cl₂

[Solve] grams Cl₂

Step 2: Identify Conversions

Avogadro's Number

[PT] Molar Mass of Cl - 35.45 g/mol

Molar Mass of Cl₂ - 2(35.45) = 70.9 g/mol

Step 3: Convert

Step 4: Check

Follow sig fig rules and round. We are given 3 sig figs.

412.072 g Cl₂ ≈ 412 g Cl₂

Answer:

780 g

Explanation:

Step 1: Given data

Moles of sodium phosphate: 4.76 moles

Step 2: Calculate the mass corresponding to 4.76 moles of sodium phosphate

To convert moles to mass, we need a conversion factor. In this case, we will use the molar mass of sodium phosphate, which is 163.94 g/mol.

4.76 mol × 163.94 g/mol = 780 g

Answer:

Subbituminous coal can form at temperatures as low as 35 to 80 °C (95 to 176 °F) while anthracite requires a temperature of at least 180 to 245 °C (356 to 473 °F).

Sub-types: Cannel coal

Child material class: Lignite

Explanation:

Answer:  The balanced equation for the given reaction is

[tex]2SO_{2}(g) + O_{2}(g) \rightarrow 2SO_{3}(g)[/tex].

Explanation:

A chemical equation which contains same number of atoms on both reactant and product side.

For example, [tex]SO_{2}(g) + O_{2}(g) \rightarrow SO_{3}(g)[/tex]

Here, number of atoms on reactant side are as follows.

Number of atoms on product side are as follows.

To balance this equation, multiply [tex]SO_{2}[/tex] by 2 on reactant side and multiply [tex]SO_{3}[/tex] by 2. Hence, the equation will be re-written as follows.

[tex]2SO_{2}(g) + O_{2}(g) \rightarrow 2SO_{3}(g)[/tex]

Here, number of atoms on reactant side are as follows.

Number of atoms on product side are as follows.

Now, there are same number of atoms on both reactant and product side. So, this equation is balanced.

Thus, we can conclude that the balanced equation for the given reaction is [tex]2SO_{2}(g) + O_{2}(g) \rightarrow 2SO_{3}(g)[/tex].

Answer:

[tex]m_{NH_3}=21.6gNH_3[/tex]

Explanation:

Hello there!

In this case, in agreement to the given chemical reaction, it is possible for us to calculate the mass of NH3 required to remove 57.0 g NO via the stoichiometry based off the 4:6 mole ratio between them:

[tex]m_{NH_3}=57.0g NO*\frac{1molNO}{30.01gNO}*\frac{4molNH_3}{6molNO} *\frac{17.03gNH_3}{1molNH_3} \\\\m_{NH_3}=21.6gNH_3[/tex]

Best regards!

Answer:

0.172 M

Explanation:

The reaction for the first titration is:

First we calculate how many HCl moles reacted, using the given concentration and volume:

As one HCl mol reacts with one NaOH mol, there are 3.704 NaOH mmoles in 25.0 mL of solution. With that in mind we determine the NaOH solution concentration:

As for the second titration:

We determine how many NaOH moles reacted:

Then we convert NaOH moles into H₃PO₄ moles, using the stoichiometric coefficients:

Finally we determine the H₃PO₄ solution concentration:

The reaction in which carbon combines with sulfur to form carbon

disulfide. Is

In a chemical reaction, bonds between molecules of the reactant are broken and new bonds between molecules of the product are established to create a new substance.

Chemical reactions occur all around us, including in our body's digestion of food and the creation of the sunlight's light. Understanding physical and chemical changes is crucial before starting any chemical reactions.

Sulfur and carbon combine to form carbon disulfide in an endothermic reaction that absorbs 92 kJ/mol of heat.

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Answer:

1116g

Explanation:

We'll convert moles O2 -> moles of Na2O -> grams of Na2O.

Based on our balanced equation, we have 1 mole of O2 for every 2 moles of Na2O. This is our mole to mole ratio.

9 mol O2 x [tex]\frac{2 mol Na2O}{1 mol O2}[/tex] = 18 mol Na2O

We can convert mols -> grams using the molar mass of Na2O- 62g.

18 mol Na2O x [tex]\frac{62g Na2O}{1 mol}[/tex] = 1116g

Answer:c

Explanation:yes

Answer:

0.0010 M of HC2H302(aq)

Answer:

2 NH₃(g) + 2 O₂(g) ⇒ N₂O(g) + 3 H₂O(l)   ΔH° = -684 kJ

Explanation:

Let's consider the unbalanced equation that occurs when NH₃(g) reacts with O₂(g) to form N₂O(g) and H₂O(l).

NH₃(g) + O₂(g) ⇒ N₂O(g) + H₂O(l)

We will begin balancing N atoms by multiplying NH₃(g) by 2.

2 NH₃(g) + O₂(g) ⇒ N₂O(g) + H₂O(l)

Then, we will balance H atoms by multiplying H₂O(l) by 3.

2 NH₃(g) + O₂(g) ⇒ N₂O(g) + 3 H₂O(l)

Finally, we will get the balanced equation by multiplying O₂(g) by 2.

2 NH₃(g) + 2 O₂(g) ⇒ N₂O(g) + 3 H₂O(l)

Since 342 kJ of energy are evolved for each mole of NH₃(g), and there are 2 moles of NH₃(g) in the balanced equation, the heat evolved will be2 × 342 kJ = 684 kJ. By convention, when heat is evolved, it takes a negative sign. The balanced thermochemical equation is:

2 NH₃(g) + 2 O₂(g) ⇒ N₂O(g) + 3 H₂O(l)   ΔH° = -684 kJ

Answer:

Explanation:

2 H₂S(g) +S0₂(g) =  3 S(s) +  2H₂0(g)

2 x 34 g     64 g        3 x 32 g

68 g of  H₂S reacts with 64 g of S0₂

3.89 g of H₂S reacts with 64 x 3 .89 / 68 g of S0₂

3.89 g of H₂S reacts with 3.66  g of S0₂

S0₂ given is 4.11 g , so it is in excess .

Hence H₂S is limiting reagent .

68 g of  H₂S reacts with  S0₂ to give 96 g of Sulphur

3.89 g of  H₂S reacts with  S0₂ to give 96 x 3.89 / 68 g of Sulphur

3.89 g of  H₂S reacts with  S0₂ to give 96 x 3.89 / 68 g of Sulphur

5.49 g of Sulphur is produced .

Actual yield is 4.89

percentage yield = 4.89 x 100 / 5.49

= 89 % .  

Considering the reaction stoichiometry and the definition of percent yield:

a. H₂S will be the limiting reagent.

b. the maximum mass of sulfur that can be produced in the reaction is 5.49 grams.

c. the percent yield of the reaction is 89%.

The balanced reaction is:

2 H₂S(g) + SO₂(g) → 3 S(s) +  2 H₂O(g)

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

The molar mass of each compound is:

So, by reaction stoichiometry, the following amounts of mass of each compound participate in the reaction:

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

To determine the limiting reagent, it is possible to use a simple rule of three as follows: if by stoichiometry 64 grams of SO₂ reacts with 68 grams of H₂S, 4.11 grams of SO₂ react with how much mass of H₂S?

[tex]mass of H_{2} S=\frac{4.11 grams of SO_{2}x 68 grams of H_{2} S }{64 grams of SO_{2}}[/tex]

mass of H₂S= 4.37 grams

But 4.37 moles of H₂S are not available, 3.89 grams are available. Since you have less mass than you need to react with 4.11 grams of SO₂, H₂S will be the limiting reagent.

Using the limiting reagent, you can apply the following rule of three: if by stoichiometry 68 grams of H₂S produce 96 grams of S, 3.89 grams of H₂S will produce how much mass of S?

[tex]mass of S=\frac{96 grams of Sx 3.89 grams of H_{2} S }{68 grams of H_{2}S}[/tex]

mass of S= 5.49 grams

So, the maximum mass of sulfur that can be produced in the reaction is 5.49 grams.

The amount of product that is obtained when all the limiting reagent reacts.  This is called the theoretical yield of the reaction. That is, the theoretical yield is the maximum amount of product that can be produced in a reaction.

On the other hand, the actual yield is the amount of product actually obtained from a reaction.

The percent yield determines the efficiency of the  reaction, and describes the ratio of the actual yield to the theoretical yield:

[tex]percent yield=\frac{actual yield}{theoretical yield}x100[/tex]

In this case, you know:

So, the percent yield can be calculated as:

[tex]percent yield=\frac{4.89 grams}{5.49 grams}x100[/tex]

Solving:

percent yield= 89%

Finally, the percent yield of the reaction is 89%.

Learn more about reaction stoichiometry:

Answer:

3.67

Explanation:

Step 1: Write the balanced equation

CO₂(g) + H₂(g) = CO(g) + H₂O(g)

Step 2: Calculate the value of the pressure equilibrium constant (Kp)

The concentration equilibrium constant (Kc) is 3.67.

We can calculate the value of the pressure equilibrium constant using the following expression.

[tex]Kp = Kc \times (R \times T)^{\Delta n(g)}[/tex]

where,

R: ideal gas constant

T: absolute temperature

Δn(g): moles of gaseous products - moles  of gaseous reactants

Δn(g) = 2 mol - 2 mol = 0

Then,

Kp = Kc × (R × T)⁰ = Kc = 3.67

Answer:

What above data?

Explanation:

There is no data to be seen here.

Explanation:

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Answer:

C₇H₁₆ + 32CoF₃ —> C₇F₁₆ + 16HF + 32CoF₂

Explanation:

C₇H₁₆ + CoF₃ —> C₇F₁₆ + HF + CoF₂

The above equation can be balance as illustrated below:

C₇H₁₆ + CoF₃ —> C₇F₁₆ + HF + CoF₂

There are 16 atoms of H on the left side and 1 atom on the right side. It can be balance by writing 16 before HF as shown below:

C₇H₁₆ + CoF₃ —> C₇F₁₆ + 16HF + CoF₂

There are 3 atoms of F on the left side and a total of 34 atoms on the right side. It can be balance by writing 32 before CoF₃ and 32 before CoF₂ as shown below:

C₇H₁₆ + 32CoF₃ —> C₇F₁₆ + 16HF + 32CoF₂

Now, the equation is balanced.

Answer: Hewo, there!

All of the above wold be my answer

Explanation:

Although many factors combine to influence weather, the four main ones are solar radiation, the amount of which changes with Earth's tilt, orbital distance from the sun and latitude, temperature, air pressure and the abundance of water.

Hope this helps you!!

Have a great day

Answer:25,06 kJ of energy must be added to a 75 g block of ice.

ΔHfusion(H₂O) = 6,01 kJ/mol.

T(H₂O) = 0°C.

m(H₂O) = 75 g.

n(H₂O) = m(H₂O) ÷ M(H₂O).

n(H₂O) = 75 g ÷ 18 g/mol.

n(H₂O) = 4,17 mol.

Q = ΔHfusion(H₂O) · n(H₂O)

Q = 6,01 kJ/mol · 4,17 mol

Q = 25,06 kJ.

Explanation: