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Lilit [14]
3 years ago
5

What were the learning goals of this lab experiment? Check all that apply.

Chemistry
2 answers:
Mice21 [21]3 years ago
7 0
All four answers are right 100%.
8090 [49]3 years ago
4 0

Answer: the second part is Hess

Explanation:

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What is the percentage yield of O2 if 12.3 g of KClO3 (molar mass 123 g) is decomposed to produce 3.2 g of O2 (molar mass 32 g)
My name is Ann [436]

Answer:

The percentage yield of O2 is 66.7%

Explanation:

Reaction for decomposition of potassium chlorate is:

2KClO₃ →  2KCl  +  3O₂

The products are potassium chloride and oxygen.

Let's find out the moles of chlorate.

Mass / Molar mass = Moles

12.3 g / 123 g/mol = 0.1 mol

So ratio is 2:3, 2 moles of chlorate produce 3 mol of oxygen.

Then, 0.1 mol of chlorate may produce (0.1  .3)/ 2 = 0.15 moles

Let's convert the moles of produced oxygen, as to find out the theoretical yield.

0.15 mol . 32 g/ 1mol = 4.8 g

To calculate the percentage yield, the formula is

(Produced Yield / Theoretical yield) . 100 =

(3.2g / 4.8g) . 100 = 66.7 %

8 0
3 years ago
Suppose these substance were placed in a freezer set to -50 grades celsius. Which substance would become a liquid. Clorine, Merc
Vadim26 [7]
Chlorine would become a liquid. Its boiling point is around -34 Celsius so at any temperature below that it would be liquid.
5 0
3 years ago
Based on the following unbalanced reaction. how many moles of U can be 2 produced when you produce 3 moles of Z?
oee [108]

Answer:

9

Explanation:

3 0
2 years ago
Which of the following definitions describes a chemical hazard?
Monica [59]
I think it would be A because hazardous waste would most likely be found in dust, fumes etc. I'm not sure though.
7 0
3 years ago
Read 2 more answers
What term is used for the chemical composition of a compound​
postnew [5]

Relative molecular mass or RMM is the answer.

4 0
3 years ago
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