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LUCKY_DIMON [66]
4 years ago
6

Which of these statements correctly compares probeware (such as an electronic temperature probe) to traditional analog tools (su

ch as a liquid-based thermometer)?
Chemistry
2 answers:
svet-max [94.6K]4 years ago
7 0
<span>Measurements by traditional analog tools are less prone to experimental error.</span>
GaryK [48]4 years ago
4 0

yeah the answer above is wrong,

Out of the four choices:

Which of these statements correctly compares probeware (such as an electronic temperature probe) to traditional analog tools (such as a liquid-based thermometer)?

A. Measurements by traditional analog tools are good to a larger number of significant figures.

B. Measurements by traditional analog tools are less prone to experimental error.

C. Probeware is typically very difficult to transport.

D. Probeware is useful for obtaining many measurements in rapid   succession.

B is wrong, I'd guess A or D. Hope this helps someone.

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If 16.0 grams of aluminum oxide were actually produced, what is the percent yield of the reaction below given that you start wit
Svetllana [295]

Answer: The percent of yield is 50.03%.

Explanation:

First, we need to balance the equation:

4Al + 3O_{2} ⇒ 2Al_{2}O_{3}

We need to remember that the chemical equations are written in moles, so we have to convert the amounts in grams to moles, using the molecular weight of every compound: Al2O3 (101.96 g/mol), Al (29.98 g/mol) and O2 (31.99 g/mol).

In consequence, the amounts in moles of every compound will be:

16 gAl_{2}O_{3} * \frac{1 mol}{101.96 g} =0.157 mol Al_{2}O_{3}

10 g Al * \frac{1mol}{29.98 g}= 0.333 mol Al

19 g O_{2}*\frac{1 mol}{31.99 g} =0.594 mol O_{2}

Now, we have to find out which is the limit reagent or in other words, which of the reagents will be consumed first, taking into account the stoichiometric ratio of the balanced equation:

0.333 mol Al * \frac{2 mol Al_{2}O_{3}}{4 mol Al} =0.1665 mol Al_{2}O_{3}

0.594 mol O_{2} * \frac{2 mol Al_{2}O_{3}}{3 mol O_{2}} =0.396 mol Al_{2}O_{3}

As you can see, the maximum amount (theoretically) of Al2O3 that can be produced is 0.1665 mol.

Finally, we have to use the yield formula to calculate the percent yield of the reaction:

Percent of yield = \frac{actual yield}{theoretical yield} * 100 = \frac{0.157 mol Al_{2}O_{3}}{0.1665 mol Al_{2}O_{3}} * 100 = 94.25

Therefore, the percent of yield is 50.03%.

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3 years ago
What is inorganic chemistry.
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Answer:the branch of chemistry that deals with inorganic compounds

Explanation:

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Answer:

LOL i belive its 200 because i did this exact same thing yesterday for homework and got it right so yeah, it should work. if it doesnt im sorry! but yeah XD sub to my yt channel too! DB_PLAYS <3

Explanation:

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Explanation:

to remind people that atoms were

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(2) The electron configuration of nitrogen is 1s22s²2p3​
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i don't know this question answer

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