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2 years ago

Sedimentary rocks formed from the remains of once-living things are

2 answers:

8 0

The correct option is D. This type of rock is called biologic sedimentary rock. It is formed from accumulation of dead living things which have been compressed and cemented together to form a rock.

Please advise if this is your complete question entirely? If yes, then your correct answer is provided above.

Sedimentary rocks formed from the remains of once-living things are ____.
a. metamorphic
c. organic
b. detrital
d. none of the above

Ivenika [448]2 years ago

4 0

The correct option is D. This type of rock is called biologic sedimentary rock. It is formed from accumulation of dead living things which have been compressed and cemented together to form a rock.

Please advise if this is your complete question entirely? If yes, then your correct answer is provided above.

Sedimentary rocks formed from the remains of once-living things are ____.

a. metamorphic

c. organic

b. detrital

d. none of the above

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Match these items with their examples.

postnew [5]

Salt=compound, soda=liquid solution, aluminum foil=element, milk=colloid,
steel=solid solution

8 0

3 years ago

Read 2 more answers

What is the molarity (molar concentration, unit = M) of K+ found in 200 mL 0.2 M K2HPO4 solution?

enyata [817]

Answer:

0.4 M

Explanation:

The process that takes place in an aqueous K₂HPO₄ solution is:

K₂HPO₄ → 2K⁺ + HPO₄⁻²

First we calculate how many K₂HPO₄ moles are there in 200 mL of a 0.2 M solution:

200 mL * 0.2 M = 40 mmol K₂HPO₄

Then we convert K₂HPO₄ moles into K⁺ moles, using the stoichiometric coefficients of the reaction above:

40 mmol K₂HPO₄ * $\frac{2mmolK^+}{1mmolK_2HPO_4}$ = 80 mmol K⁺

Finally we divide the number of K⁺ moles by the volume, to calculate the molarity:

80 mmol K⁺ / 200 mL = 0.4 M

5 0

2 years ago

Waves move out through the ground from the source of an earthquake. True ► False

goblinko [34]

I believe the answer would be true

3 0

3 years ago

A sample of helium gas has a pressure of 1.20 atm at 22°c. at what celsius temperature will the helium reach a pressure of 2.00

sukhopar [10]

Gay-Lussac's law gives the relationship between pressure and temperature of a gas.
it states that for a fixed amount of gas of constant volume pressure is directly proportional to temperature.
P/T = k
where P - pressure, T - temperature and k - constant
$\frac{P1}{T1} = \frac{P2}{T2}$
where parameters for the first instance are on the left side and parameters for the second instance are on the right side of the equation.
temperature should be in the kelvin scale,
T1 = 22 °C + 273 = 295 K
substituting the values in the equation
$\frac{1.20atm}{295 K} = \frac{2.00 atm}{T}$
T = 492 K
new temperature - 492 - 273 = 219 °C

5 0

3 years ago

Consider the balanced equation for the following reaction:

Bad White [126]

Answer: The theoretical yield of the lithium chlorate is 1054.67 grams

Explanation:

To calculate the mass for given number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Actual moles of lithium chlorate = 9.45 moles

Molar mass of lithium chlorate = 90.4 g/mol

Putting values in above equation, we get:

$9.45mol=\frac{\text{Actual yield of lithium chlorate}}{90.4g/mol}\\\\\text{Actual yield of lithium chlorate}=(9.45mol\times 90.4g/mol)=854.28g$

To calculate the theoretical yield of lithium chlorate, we use the equation:

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

Actual yield of lithium chlorate = 854.28 g

Percentage yield of lithium chlorate = 81.0 %

Putting values in above equation, we get:

$81=\frac{854.28g}{\text{Theoretical yield of lithium chlorate}}\times 100\\\\\text{Theoretical yield of lithium chlorate}=\frac{854.28\times 100}{81}=1054.67g$

Hence, the theoretical yield of the lithium chlorate is 1054.67 grams

7 0

2 years ago