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Leto [7]
3 years ago
12

How many significant figures are in each measurement? 0.00052 m

Chemistry
2 answers:
NikAS [45]3 years ago
8 0
All the measurement contain two significant figures
leonid [27]3 years ago
6 0

a. 0.00052 m


Answer: two significant figures.


Explanation:


The zeros to the left of 52 do not count as signficant figures.


Only, 5 and 2 are significant figures.


b. 9.8 x 10⁴ g


Answer: two significant figures.


Explanation:


Both 9 and 8 count as significant figures. Here there are not additional zeros that might confuse you.



c. 5.050 mg


Answer: four significant figures.


Explanation:


The zeros to the right count as signficiant figjres. So here, 5, 0, 5, and 0 are the significant figures.



d. 8700 ml


Answer: two signficant figures.


Explanation:


Since the two zeros to the right are used to determine the place value of 87, you cannot count them as significant figures. Here, only 8 and 7 are significant figures.

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Due to the fact that ice is less thick than liquid water, the phase diagram of water has an odd melting point that drops with pressure. Carbon dioxide cannot exist as a liquid at atmospheric pressure, according to the phase diagram of the gas. Thus, gaseous carbon dioxide directly sublimes from solid carbon dioxide.

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3 0
1 year ago
When a 0.245-g sample of benzoic acid is combusted in a bomb calorimeter, the temperature rises 1.643 ∘C . When a 0.260-g sample
sveticcg [70]

Answer:

The heat of combustion per moles of caffeine is 4220 kJ/mol

Explanation:

Step 1: Data given

⇒ When  benzoic acid sample of 0.245 grams is burned the temperature rise is 1.643 °C

⇒ When 0.260 gram of caffeine is burned, the temperature rise is 1.436 °C

⇒ Heat of combustion of benzoic acid = 26.38 kJ/g

<u>Step 2:</u> Calculate the heat released: for combustion of benzoic acid

0.245 g benzoic acid *  26.38 kJ/g = 6.4631 kJ

<u>Step 3</u>: Calculate the heat capacity of the calorimeter:

c = Q/ΔT

Q = 6.4631 kJ   / 1.643°C = 3.934 kJ/ °C

<u>Step 4:</u> Calculate moles of a 0.260 g sample of caffeine:

Moles caffeine = Mass caffeine / Molar mass caffeine

0.260 grams/ 194.19 g/mol  = 0.0013389 moles

Step 5: Calculate heat released: for combustion of caffeine

Q = c * ΔT

Q = 3.934 kJ/°C * 1.436 °C = 5.65 kJ

Step 6: Calculate the heat of combustion per mole of caffeine  

5.65 kJ  /  0.0013389 moles = 4219.9 kJ/mol  ≈ 4220 kJ/mol

The heat of combustion per moles of caffeine is 4220 kJ/mol

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