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Dmitry_Shevchenko [17]

4 years ago

7

Which sphere exists because of there is liquid iron as part of the earth's core? A.hydrosphere B.atmosphere C.magnetosphere D.li

thosphere

1 answer:

Naily [24]4 years ago

5 0

The answer is lithosphere

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Ned help with this question

tia_tia [17]

Answer:

135.6

Explanation:

12 * 11.3 = 135.6

To find the mass you have to multiply the density and volume together

If you already have the mass you divide the mass by either the density or volume

8 0

3 years ago

Describe the silica tetrahedron

Travka [436]

Answer:

This fundamental structural unit consists of a silicon cation surrounded by four oxygen anions giving it four negative charges. It is found in all silicate minerals (ie. amphibole, olivine, pyroxene, quartz, feldspar, etc.). The silica tetrahedra may be arranged in chains (ex: pyroxenes), double chains (ex. amphiboles), sheets (ex: micas), and frameworks (ex: quartz, feldspars), forming the basic structure of the planet.

4 0

3 years ago

What is the pressure of a mixture of 0.200 g of H2, 1.00 g of N2 , and 0.820 g of Ar in a container with a volume of 2.00 L at 2

alexdok [17]

Answer:

P(mixture) = 1.92 atm

Explanation:

Given data:

Mass of H₂ = 0.200 g

Mass of N₂ = 1.00 g

Mass of Ar = 0.820 g

Volume = 2 L

Temperature = 20°C

Pressure of mixture = ?

Solution:

Pressure of hydrogen:

Number of moles of hydrogen = mass / molar mass

Number of moles of hydrogen = 0.200 g / 2 g/mol

Number of moles of hydrogen = 0.1 mol

P = nRT / V

P = 0.1 mol× 0.0821 atm. L.mol⁻¹ .k⁻¹ × 293 K / 2L

p = 2.41 atm. L /2 L

P = 1.2 atm

Pressure of nitrogen:

Number of moles of nitrogen = mass / molar mass

Number of moles of nitrogen = 1 g / 28 g/mol

Number of moles of nitrogen = 0.04 mol

P = nRT / V

P = 0.04 mol× 0.0821 atm. L.mol⁻¹ .k⁻¹ × 293 K / 2L

p = 0.96 atm. L /2 L

P = 0.48 atm

Pressure of argon:

Number of moles of argon = mass / molar mass

Number of moles of argon = 0.820 g / 40 g/mol

Number of moles of argon = 0.02 mol

P = nRT / V

P = 0.02 mol× 0.0821 atm. L.mol⁻¹ .k⁻¹ × 293 K / 2L

p = 0.48 atm. L /2 L

P = 0.24 atm

Total pressure of mixture:

P(mixture) = pressure of hydrogen + pressure of nitrogen + pressure of argon

P(mixture) = 1.2 atm + 0.48 atm + 0.24 atm

P(mixture) = 1.92 atm

5 0

3 years ago

A 3.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of

andrew-mc [135]

Answer: The molecular formula for the given organic compound X is $C_6H_{8}O_7$

Explanation:

We are given:

Mass of $CO_2=4.13g$

Mass of $H_2O=1.13g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 4.13 g of carbon dioxide, = $\frac{12}{44}\times 4.13=1.13g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 1.13 g of water, $\frac{2}{18}\times 1.13=0.125g$ of hydrogen will be contained.

Mass of oxygen in the compound = (3.00) - (1.13+ 0.125) = 1.75 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{1.13g}{12g/mole}=0.094moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.125g}{1g/mole}=0.125moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{1.75g}{16g/mole}=0.109moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles

For Carbon = $\frac{0.094}{0.094}=1$

For Hydrogen = $\frac{0.125}{0.094}=1.33$

For Oxygen = $\frac{0.109}{0.094}=1.16$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 1: 1.33: 1.16

Converting them into whole number ratios by multiplying by 6:

The ratio of C : H : O = 6: 8: 7

Hence, the empirical formula for the given compound is $C_6H_8O_7$

Empirical mass = $6\times 12+8\times 1+7\times 16=192g$

The equation used to calculate the valency is :

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

Putting values in above equation, we get:

$n=\frac{192g/mol}{192g/mol}=1$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_6H_8O_7\times 1=C_6H_{8}O_7$

Thus molecular formula for the given organic compound X is $C_6H_{8}O_7$

7 0

3 years ago

Why did biologist in the 1960s recommend reintroducing wolves to yellow stone

Montano1993 [528]

D), because any GOOD <span>environmentalist doesn't CARE about tourist's.

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6 0

4 years ago