2 years ago

Which of the following is most likely a homogeneous mixture?

Chemistry

2 answers:

Dmitry [639]2 years ago

8 0

Answer:

D)A vanilla milkshake

Explanation:

natali 33 [55]2 years ago

7 0

D) A vanilla milkshake.

That’s the case because you can’t physically separate the different posts that make up the mixture.

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1. Intermolecular forces do not have any effect on determining the physical properties of substances such as surface tension and

Scilla [17]

Answer:

1)false

2) false

3)True

4)True

5) false

6)false

7) true

8) d

9)false

10) b

5 0

2 years ago

What is the molarity of the potassium hydroxide if 25.25 mL of KOH is required to neutralize 0.500 g of oxalic acid, H2C2O4? H2C

Greeley [361]

Answer:

0.444 mol/L

Explanation:

First step is to find the number of moles of oxalic acid.

n(oxalic acid) = $\frac{0.5g}{90.03 g/mol} = 5.5537*10^{-3} mol\\$

Now use the molar ratio to find how many moles of NaOH would be required to neutralize $5.5537*10^{-3} mol\\$ of oxalic acid.

n(oxalic acid): n(potassium hydroxide)

1 : 2 (we get this from the balanced equation)

$5.5537*10^{-3} mol\\$ : x

x = 0.0111 mol

Now to calculate what concentration of KOH that would be in 25 mL of water:

$c = \frac{number of moles}{volume} = \frac{0.0111}{0.025} = 0.444 mol/L$

5 0

3 years ago

Given the balanced equation, calculate the mass of product that can be prepared from 2.10 g of zinc metal. 2Zn(s)+O2(g)→2ZnO(s)

vazorg [7]

Botox & Glade Juice w/ Apple Cider Vinegar

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3 years ago

A chemist determined by measurements that 0.050 moles of aluminum participated in a chemical reaction. Calculate the mass of alu

Law Incorporation [45]

Answer:

13.5 g

Explanation:

This question is solved easily if we remember that the number of moles is obtained by dividing the mass into the atomic weight or molar mass depending if we are referring to elements or molecules.

Therefore, the mass of aluminum in the reaction will the 0.050 mol Al times the atomic weight of aluminum.

number of moles = n = mass of Al / Atomic Weight Al

⇒ mass Al = n x Atomic Weight Al = 0.050 mol x 27 g mol⁻¹

= 13.5 g

We have three significant figures in 0.050 and therefore we should have three significant figures in our answer.

8 0

3 years ago

In the equation: 23491Pa → 234 92U + X The X represents a

Bad White [126]

Beta particle in the reaction

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3 years ago