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Ivan
3 years ago
8

Select all that apply. Which of the following measurements have 3 significant figures? 0.0882 m 0.8820 m 8,820 m 882.0 m

Chemistry
2 answers:
mixer [17]3 years ago
4 0

Answer:

0.0882

8,820

Explanation:

0.0882  is one . The significant figures are 882. We ignore the leading zeroes.

0.8820 has 4 significant figures.

8.820 also has 3 significant figures (we do not count the trailing zero).

882.0 has 4 significant figures.

MatroZZZ [7]3 years ago
3 0

8820 and 0.0882 have three sig figs

When a number has zeros in it I struggled a lot to determine if it what a sig fig or not. This is how I remember it:

If a zero is a sandwich between normal numbers it IS a sig fig

Zero's after the decimal ARE sig figs

***IMPORTANT! There is an exception to this one which I'll talk about next :)

Leading zeros (I believe that is what they are called) are NOT sig figs. This would be like the zeros in the following numbers:

0.2

0.03

0.000000000000000000006

If there are zeros after normal numbers and there is NO DECIMAL it is NOT a sig fig.  This would be like the zeros in the following numbers:

630

3, 000

536, 329,600,000

Take a look at the other numbers:

0.8820 <<<This has 4 sig. figs.

882.0 <<<This has 4 sig. figs.

***Remember that if there is a pure decimal the zero in front of the decimal is NOT a sig fig and just a place holder. It isn't necessary and can always be taken away

Hope this made sense and helped!!!

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How many Joules are released to cool 250.0 grams of liquid water from 100°C to 0°C? The specific heat of water is 4.180 J/g.C.
nlexa [21]

\bold{\huge{\orange{\underline{ Solution}}}}

\bold{\underline{ Given :- }}

  • <u>We </u><u>have </u><u>250g </u><u>of </u><u>liquid </u><u>water </u><u>and </u><u>it </u><u>needs </u><u>to </u><u>be </u><u>cool </u><u>at </u><u>temperature </u><u>from </u><u>1</u><u>0</u><u>0</u><u>°</u><u> </u><u>C </u><u>to </u><u>0</u><u>°</u><u> </u><u>C</u>
  • <u>Specific </u><u>heat </u><u>of </u><u>water </u><u>is </u><u>4</u><u>.</u><u>1</u><u>8</u><u>0</u><u>J</u><u>/</u><u>g</u><u>°</u><u>C</u>

\bold{\underline{ To \: Find :- }}

  • <u>We </u><u>have </u><u>to </u><u>find </u><u>the</u><u> </u><u>total</u><u> </u><u>number </u><u>of </u><u>joules </u><u>released</u><u>. </u>

\bold{\underline{ Let's \:Begin:- }}

<u>We </u><u>know </u><u>that</u><u>, </u>

Amount of heat energy = mass * specific heat * change in temperature

<u>That </u><u>is, </u>

\sf{\red{ Q = mcΔT }}

<u>Subsitute </u><u>the </u><u>required </u><u>values </u><u>in </u><u>the </u><u>above </u><u>formula </u><u>:</u><u>-</u>

\sf{ Q = 250 × 4.180 ×(0 - 100 )}

\sf{ Q = 250 × 4.180 × - 100 }

\sf{ Q = 250 × - 418}

\sf{\pink{ Q = - 104,500 J }}

Hence, 104,500 J of heat is released to cool 250 grams of liquid water from 100° C to 0° C.

\bold{\underline{ Now :- }}

<u>We </u><u>have </u><u>to </u><u>tell </u><u>whether </u><u>the </u><u>above </u><u>process </u><u>is </u><u>endothermic </u><u>or </u><u>exothermic </u><u>:</u><u>-</u>

Here, In the above process ΔT is negative and as a result of it Q is also negative that means above process is Exothermic

  • <u>Exothermic </u><u>process </u><u>:</u><u>-</u><u> </u><u>It </u><u>is </u><u>the </u><u>process </u><u>in </u><u>which </u><u>heat </u><u>is </u><u>evolved </u><u>. </u>
  • <u>Endothermic </u><u>process </u><u>:</u><u>-</u><u> </u><u>It </u><u>is </u><u>the </u><u>process </u><u>in </u><u>which </u><u>heat </u><u>is </u><u>absorbed </u><u>.</u>
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