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3 years ago

What is the chemical name of the compound K2SO4? Use the list of polyatomic ions and the periodic table to help you answer.

Chemistry

2 answers:

Inga [223]3 years ago

8 0

Answer: Option (B) is the correct answer.

Explanation:

The given compound is $K_{2}SO_{4}$ , that is, it contains potassium $(K^{+})$ and sulphate $(SO^{2-}_{4})$ ions.

Charge on a sulphate ion is -2 and charge on two potassium ions is +2. Therefore, according to cross multiplication method it results in the formation of $K_{2}SO_{4}$ .

Thus, we can conclude that chemical name of the compound is potassium sulfate.

Ket [755]3 years ago

6 0

potassium sulfate or A because K2 is potassium and SO4 is sulfate

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3 years ago

Write the Formulas for these ionic compounds:

Alinara [238K]

Answer:

<h2>1. Tin(IV) oxide</h2>

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Melting point: 1,630 °C

Density: 6.95 g/cm³

<h2>2. Aluminum oxide</h2>

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Formula: Al₂O₃

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Boiling point: 2,977 °C

ChemSpider ID: 14086

ChemSpider ID: 26988

<h2>3. Silver sulfide</h2>

Silver sulfide is an inorganic compound with the formula Ag ₂S. A dense black solid, it is the only sulfide of silver. It is useful as a photosensitizer in photography. It constitutes the tarnish that forms over time on silverware and other silver objects.

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IUPAC ID: Copper(II) sulfate

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<h2>5. Potassium carbonate</h2>

Potassium carbonate is the inorganic compound with the formula K₂CO₃. It is a white salt, which is soluble in water. It is deliquescent, often appearing as a damp or wet solid. Potassium carbonate is mainly used in the production of soap and glass.

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Explanation:

Hope it is helpful....

4 0

3 years ago

A 32 L samples of xenon gas at 10°C is expanded to 35 L. Calculate the final temperature.

morpeh [17]

Answer:

Final Temperature = 36.54 ⁰C

Explanation:

Lets suppose the gas is acting ideally, then according to Charle's Law, "<em>The volume of a fixed mass of gas at constant pressure is directly proportional to the absolute temperature</em>". Mathematically for initial and final states the relation is as follow,

V₁ / T₁ = V₂ / T₂

Data Given;

V₁ = 32 L

T₁ = 10 °C = 283.15 K ∴ K = °C + 273.15

V₂ = 35 L

T₂ = ??

Solving equation for T₂,

T₂ = V₂ × T₁ / V₁

Putting values,

T₂ = (35 L × 283.15 K) ÷ 32 L

T₂ = 309.69 K ∴ ( 36.54 °C )

Result:

As the volume is increased from 32 L to 35 L, therefore, the temperature must have increased from 10 °C to 36.54 °C.

3 0

4 years ago

What is the molarity of a solution that contains 122g of MgSO4 n 3.5L of solution?

Semmy [17]

Answer:

0.29mol/L or 0.29moldm⁻³

Explanation:

Given parameters:

Mass of MgSO₄ = 122g

Volume of solution = 3.5L

Molarity is simply the concentration of substances in a solution.

Molarity = number of moles/ Volume

>>>>To calculate the Molarity of MgSO₄ we find the number of moles using the mass of MgSO₄ given.

Number of moles = mass/ molar mass

Molar mass of MgSO₄:

Atomic masses: Mg = 24g

S = 32g

O = 16g

Molar mass of MgSO₄ = [24 + 32 + (16x4)]g/mol

= (24 + 32 + 64)g/mol

= 120g/mol

Number of moles = 122/120 = 1.02mol

>>>> From the given number of moles we can evaluate the Molarity using this equation:

Molarity = number of moles/ Volume

Molarity of MgSO₄ = 1.02mol/3.5L

= 0.29mol/L

IL = 1dm³

The Molarity of MgSO₄ = 0.29moldm⁻³

8 0

3 years ago

PLEASE HELP!!

grandymaker [24]

Answer:

1. 136 °C.

2. 0.21 atm.

Explanation:

1. Determination of the new temperature in °C.

Initial volume (V1) = 1.35L

Final volume (V2) = 1.95L

Initial temperature (T1) = 283 K

Final temperature (T2) =...?

Using the Charles' law equation, the new temperature of the gas can be obtained as follow:

V1 /T1 = V2 /T2

1.35/283 = 1.95/T2

Cross multiply

1.35 × T2 = 283 × 1.95

1.35 × T2 = 551.85

Divide both side by 1.35

T2 = 551.85/1.35

T2 = 408.8 ≈ 409 K

Finally, we shall convert 409 K to °C. This can be obtained as follow:

T (°C) = T(K) – 273

T(K) = 409 K

T (°C) = 409 – 273

T (°C) = 136 °C

Therefore, the new temperature of the gas is 136 °C.

2. Determination of the new pressure.

Initial pressure (P1) = 1.34 atm

Initial volume (V1) = 267 mL

Final volume (V2) = 1.67 L

Final pressure (P2) =.?

Next, we shall convert 1.67 L to millilitres (mL). This can be obtained as follow:

1 L = 1000 mL

Therefore,

1.67 L = 1.67 L × 1000 mL / 1 L

1.67 L = 1670 mL

Therefore, 1.67 L is equivalent to 1670 mL.

Finally, we shall determine the new pressure of the gas as follow:

Initial pressure (P1) = 1.34 atm

Initial volume (V1) = 267 mL

Final volume (V2) = 1670 mL

Final pressure (P2) =.?

P1V1 = P2V2

1.34 × 267 = P2 × 1670

357.78 = P2 × 1670

Divide both side by 1670.

P2 = 357.78 / 1670

P2 = 0.21 atm.

Therefore, the new pressure of the gas is 0.21 atm.

3 0

3 years ago