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2 years ago

- A 300g sample of CaCO3 was heated until 10 L of CO2 was collected

Chemistry

1 answer:

elixir [45]2 years ago

6 0

Answer:

C.12.3%. you need to use pv=nRT (ideal gas law)

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Using a graduated cylinder, fill a 600 mL beaker with 100 mL of water.

fomenos

Answer:

Temperature of water: 3

Reaction time: 138.5

Explanation:

Your welcome

5 0

3 years ago

Read 2 more answers

An object has a density that is greater than the density of water. How could you make it float? Explain by giving a real-life ex

vladimir1956 [14]

Answer:

Put it on a ship or an aerogel

Explanation:

You can use an aerogel, a synthetic porous ultralight material. The aerogel can support a mass many times greater than their own.

Even simpler, you can put the object on board a ship. The ship has a smaller density than water, making it float in water.

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2 years ago

True for a group of cells is called an organ

harina [27]

False. A group of cells is called a tissue.

6 0

2 years ago

In an experiment, a compound was determined to contain 68.94% oxygen and 31.06% of an unknown element by weight. The molecular w

monitta

Answer is: the compound is B₂O₃.

ω(O) = 68.94% ÷ 100%.

ω(O) = 0.6894; percentage of oxygen in the compound.

ω(X) = 31.06% ÷ 100%.

ω(X) = 0.3106; percentage of unknown element in the compound.

If we take 69.7 grams of the compound:

M(compound) = 69.7 g/mol.

n(compound) = 69.7 g ÷ 69.7 g/mol.

n(compound) = 1 mol.

n(O) = (69.7 g · 0.6894) ÷ 16 g/mol.

n(O) = 3 mol.

M(compound) = n(O) · M(O) + n(X) · M(X).

n(X) = 1 mol ⇒ M(X) = 21.7 g/mol; there is no element with this molecular weight.

n(X) = 2 mol ⇒ M(X) = 10.85 g/mol; this element is boron (B).

8 0

2 years ago

Please this is important

ValentinkaMS [17]

Answer:

Explanation:

2C6H6 + 9O2 -> 12CO2 + 6H20

Weight of a CO2 Mol 12+ 16x2 = 44g

In 100g number of moles = 100/44= 2.2727 Moles

Number of C6H6 2moles burned when creating 12 moles of CO2

Therefore 2.2727/12 x 2 = 0.3787

3H2SO4 + 2Al(OH)3 -> Al2(SO4)3 + 6H2O

H2O weight of a 1mol is = 2+16 = 18g

2moles of Al(OH)3 cerates 6 moles of water.

3moles of sulfuric creates 6 moles of water.

5.5moles Al(OH)3 reacts with 5.5 moles of sulfuric

Therefore number of water moles = 5.5/3 x 6 = 11moles

Weight water = 11 x 18 = 198g

Cu + 2AgNO3 -> 2Ag + Cu(NO3)2

1mol of Cu produces 2moles of silver

Ag = 107.86 g/Mol

Cu = 63.54 g/Mol

In 26g Ag number of moles = (26/107.86)/2 x 63.54 = 7.658g

3K2CrO4 + 2AlPO4 -> 2K3PO4 + Al2(CrO4)3

K2CrO4 = 39x2 + 52 + 16x4 = 194g/Mol

Al2(CrO4)3 = 54 + 354 = 408g/Mol

3moles of K2CrO4 creates 1mol of Al2(CrO4)3

Therefore weight of the Al2(CrO4)3 produced by 17.5g potassium chromate

(17.5/194)/3 moles of Al2(CrO4)3 produced = 0.03moles

Al2(CrO4)3 produced = 0.03 x 408 = 12.26g

7 0

2 years ago