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3 years ago

A chef makes salad dressing by mixing oil, vinegar, and spices, as shown. Which type of matter is the salad dressing?

2 answers:

8 0

The answer is heterogeneous because if a salad is mixed by the following item it will not mix properly and we could easily separate them.

hope that helps you

have a great day!

Vika [28.1K]3 years ago

7 0

Explanation:

A mixture in which solute particles are unevenly distributed into the solvent is known as a heterogeneous mixture.

For example, oil present in vinegar will unevenly mix together.

Whereas a mixture in which solute particles are evenly distributed into the solvent is known as a homogeneous mixture.

For example, salt dissolved in water is a homogeneous mixture.

Therefore, when a salad dressing is made by a chef by mixing oil, vinegar, and spices then it is a heterogenous mixture.

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What major gases are absorb by the ocean

zysi [14]

Answer:

C) carbon dioxide and hydrigen

7 0

3 years ago

How many dm3 of oxygen at STP would be required to react completely with 38.8g of propane? (3 marks)

11Alexandr11 [23.1K]

$98.56 dm^3$ of oxygen at STP would be required to react completely with 38.8g of propane.

<u>Given that :</u>

molar mass of propane = 44 g/mol

mass of propane = 38.8 g

∴ Moles present in 38.8 g of propane = $\frac{38.8}{44}$ = 0.88 mole

<u>applying rule of balanced equations </u>

1 mole of propane = 5 moles of oxygen

0.88 mole of propane = 5 * 0.88 = 4.4 moles of oxygen

Note : volume of 1 mole of oxygen at STP = $22.4 dm^3$

∴Total volume of oxygen required at STP = 22.4 * 4.4 = $98.56 dm^3$

Hence we can conclude that the volume of oxygen at STP required to react completely $98.56 dm^3$

Learn more : brainly.com/question/16998374

5 0

2 years ago

Please help me on this I’ll give 30 points

Rufina [12.5K]

Answer:

1. 10.66 moles of Al

2. 2.5 moles of Al₂O₃

3. 143.87 g of SO₂

Explanation:

The balance chemical equation is as follow,

4 Al + 3 O₂ → 2 Al₂O₃

According to balance chemical equation,

3 moles of O₂ required = 4 moles of Al

So,

8 moles of O₂ will require = X moles of Al

Solving for X,

X = 8 mol × 4 mol / 3 mol

X = 10.66 moles of Al

According to balance chemical equation,

4 moles of Al produced = 2 moles of Al₂O₃

So,

5 moles of Al will produce = X moles of Al₂O₃

Solving for X,

X = 5 mol × 2 mol / 4 mol

X = 2.5 moles of Al₂O₃

The balance chemical equation for the oxidation of carbon disulfide is as follow;

CS₂ + 3 O₂ → CO₂ + 2 SO₂

Step 1: <u>Calculate Moles of CS₂ as;</u>

Moles = Mass / M.Mass

Moles = 85.5 g / 76.14 g/mol

Moles = 1.12 moles of CS₂

Step 2: <u>Find out moles of SO₂ as;</u>

According to balance chemical equation,

1 mole of CS₂ produced = 2 moles of SO₂

So,

1.12 moles of CS₂ will produce = X moles of SO₂

Solving for X,

X = 1.12 mol × 2 mol / 1 mol

X = 2.24 moles of SO₂

Step 3: <u>Calculate Mass of SO₂ as;</u>

Mass = Moles × M.Mass

Mass = 2.24 mol × 64.06 g/mol

Mass = 143.87 g of SO₂

4 0

3 years ago

If you were looking for transport proteins, where would you find them?

noname [10]

Answer:Transport proteins are found within the membrane itself, where they form a channel, or a carrying mechanism, to allow their substrate to pass from one side to the other.

Explanation:

7 0

3 years ago

Determine the empirical formula of the following compound if a sample contains 0.104 molK, 0.052 molC, and 0.156 molO;?

faltersainse [42]

Answer:

K₂CO₃

Explanation:

Given parameters:

Number of moles of K = 0.104mol

Number of moles of C = 0.052mol

Number of moles of O = 0.156mol

Method

From the given parameters, to calculate the empirical formula of the elements K, C and O, we reduce the given moles to the simplest fraction.

Empirical formula is the simplest formula of a compound and it differs from the molecular formula which is the actual formula of a compound.

Divide the given moles through by the smallest which is C, 0.052mol.
Then approximate values obtained to the nearest whole number of multiply by a factor to give a whole number ratio.
This is the empirical formula

Solution

Elements K C O

Number of moles 0.104 0.052 0.156

Dividing by the

smallest 0.104/0.052 0.052/0.052 0.156/0.052

2 1 3

The empirical formula is K₂CO₃

3 0

3 years ago