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algol [13]
3 years ago
6

Review the following statement.

Chemistry
1 answer:
BartSMP [9]3 years ago
5 0

Answer:

I think its either A or B.

Explanation:

The reason I don't think it can be B or C is because both have too do with thinking. Technology does not control how you think, so those should stay about the same. Technology can help prove theories and hypothesis' to be true, but they could also make more observations due to the technology they didn't have before. I believe the answer is A, but I'm not 100% sure. Good Luck, i helped as best as i thought possible.

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Given the noble gas configuration of an element: [Ar] 4s2, 3d5, what is the element?
monitta

Question

<em>Given the noble gas configuration of an element: [Ar] 4s2, 3d5, what is the element? </em>

Answer:

<em>B.) Argon</em>

Hope this helps!

6 0
2 years ago
Which reaction below represents a balanced, double replacement chemical reaction? A) C2H5OH + 3O2 → 2CO2 + 3H2O B) Rb2O + Cu(C2H
guajiro [1.7K]
Option B. <span>Rb2O + Cu(C2H3O2)2 → 2RbC2H3O2 + CuO is the correct answer. HOPE IT HELPS</span>
8 0
3 years ago
Read 2 more answers
A 3.8-mol sample of KClO3 was decomposed according to the equation. How many moles of O2 are formed assuming 100% yield?
kari74 [83]

Answer:

5.7 moles of O2

Explanation:

We'll begin by writing the balanced decomposition equation for the reaction. This is illustrated below:

2KClO3 —> 2KCl + 3O2

From the balanced equation above,

2 moles of KClO3 decomposed to produce 3 moles of O2.

Next, we shall determine the number of mole of O2 produced by the reaction of 3.8 moles of KClO3.

Since 100% yield of O2 is obtained, it means that both the actual yield and theoretical yield of O2 are the same. Thus, we can obtain the number of mole of O2 produced as follow:

From the balanced equation above,

2 moles of KClO3 decomposed to produce 3 moles of O2.

Therefore, 3.8 moles of KClO3 will decompose to produce = (3.8 × 3)/2 = 5.7 moles of O2.

Thus, 5.7 moles of O2 were obtained from the reaction.

3 0
2 years ago
What is a solution?
Keith_Richards [23]

Answer:

A !!

it a mix where everything is combined together

5 0
2 years ago
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What is the final volume of a gas (in liters) when the initial volume is 14.00 L at
8_murik_8 [283]

Answer:

V_2=1344L

Explanation:

Hello there!

In this case, since we have a problem about volume-pressure relationship, the idea here is to use the Boyle's law to calculate the final volume as shown below:

P_2V_2=P_1V_1\\\\V_2=\frac{P_2V_2}{P_1}\\

Then, we plug in the initial and final pressures and the initial volume to obtain:

V_2=\frac{14.00L*0.9600atm}{0.01000atm}\\\\V_2=1344L

Regards!

4 0
2 years ago
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