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ycow [4]
3 years ago
8

Please help-----------------------------------------------------------------------------------------------------------a scientis

t adds three drops of vinegar to a container of baking soda and notices that the baking soda begins to bubble. This is a description of what type of property used to describe a substance?
A.
reactivity
B.
density
C.
solubility
D.
conductivity
Chemistry
1 answer:
VARVARA [1.3K]3 years ago
6 0

Answer:

A

Explanation:

The type of property used to describe a substance is reactivity

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12. What is the mass number of an atom that has 4 protons, 4 electrons, and 5 neutrons?
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Answer:

9

Explanation:

mass number = protons + neutrons

= 4 + 5 = 9

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3 years ago
Predict the type of substitution mechanism predict which reaction of the pair will occur at a faster rate
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You put in a variable to substitute the unknown number.
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What is the molar mass of water (H2O)?
Sidana [21]

Answer:

The molar mass is: 18.02 g/mol.

Explanation:

  • Mass of two moles of Hydrogen atoms (H2) = 2x 1 g/mol = 2 g/mol.
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1 mole of Hydrogen= 1.01, so if we have 2 moles of it here, that would be 2.02.

1 mole of Oxygen (that's all we have here)= 16.00

Once you add the two together (2.02+16.00), you will get 18.02.

I hope this made sense! Have a great day!

3 0
3 years ago
30. The density of an unknown gas at 27°C and 2 atm pressure is equal with density of N2 gas at
Zanzabum

Answer:

Molar mass of the unknown gas is 64.6 g/mol

Explanation:

Let's think this excersise with the Ideal Gases Law.

We start from the N₂. At STP conditions we know that 1 mol of anything occupies 22.4L.

We apply: P . V = n . R . T

5 atm . V = 1 mol . 0.082 . 325K

V = (1 mol . 0.082 . 325K) / 5 atm = 5.33 L

It is reasonable to say that, if we have more pressure, we may have less volume.

As this is the volume for 1 mol of N₂, our mass is 28 g. Then, the density of the nitrogen and the unknown gas is 28 g/5.33L = 5.25 g/L

Our unknown gas has, this density at 27°C and 2 atm.

If we star from this, again: 1 mol of any gas occupy 22.4L at STP, we can calculate the volume for 1 mol at those conditions:

P₁ . V₁ / T₁ = P₂ . V₂ / T₂

1 atm . 22,4L / 273K = 2 atm . V₂ / 300K

Remember that the value for T° is Absolute (T°C + 273)

[ (1 atm . 22.4L / 273K) . 300K] / 2 atm = V₂ → 12.3L

This is the volume for 1 mol of the unknown gas at 2 atm and 27°C

We use density to determine the mass: 12.3 L . 5.25 g/L = 64.6 g

That's the molar mass: 64.6 g/mol

6 0
2 years ago
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