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Alenkasestr [34]
2 years ago
14

What is the mass in grams of 10.76 mL of acetone? When it has a density of .7857g/cm^3

Chemistry
1 answer:
kirza4 [7]2 years ago
3 0
Answer: 8.454132 grams

Explanation:

Density = (mass) / (volume)

Mass = (density) • (volume) = .7857 • 10.76 = 8.454132 grams
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Which situation best represents convection
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A hot air balloon taking off

Explanation:

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Many repeating, simple subunits are joined together. What is the most likely
Hatshy [7]

Answer:

O a polymer

Explanation:

When many repeating simple subunits are joined together, this results into a polymer.

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3 years ago
A welding torch produces a flame by burning acetylene fuel in the presence of oxygen. This flame is used to melt a metal. Which
NISA [10]

Answer:

chemical energy into thermal energy

Explanation:

The reaction taking place is as follows

2C₂H₂ + 5O₂ = 4CO₂ + 2H₂O + Heat

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5 0
3 years ago
A gas has a volume of 62.65L at O degrees Celsius and 1 atm. At what temperature in Celsius would the volume of the gas be 78.31
Anastaziya [24]

Answer:

The volume of the gas will be 78.31 L at 1.7 °C.

Explanation:

We can find the temperature of the gas by the ideal gas law equation:

PV = nRT

Where:

n: is the number of moles

V: is the volume

T: is the temperature

R: is the gas constant = 0.082 L*atm/(K*mol)

From the initial we can find the number of moles:

n = \frac{P_{1}V_{1}}{RT_{1}} = \frac{1 atm*62.65 L}{(0.082 L*atm/K*mol)*(0 + 273)K} = 2.80 moles

Now, we can find the temperature with the final conditions:

T_{2} = \frac{P_{2}V_{2}}{nR} = \frac{612.0 mmHg*\frac{1 atm}{760 mmHg}*78.31 L}{2.80 moles*0.082 L*atm/(K*mol)} = 274.7 K

The temperature in Celsius is:

T_{2} = 274.7 - 273 = 1.7 ^{\circ} C

Therefore, the volume of the gas will be 78.31 L at 1.7 °C.

I hope it helps you!            

8 0
3 years ago
I need help please.​
murzikaleks [220]

Answer:

3

Explanation:

4 0
3 years ago
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