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4 years ago

Please select the word from the list that best fits the definition

Chemistry

1 answer:

Nastasia [14]4 years ago

6 0

Answer:

The answer is B(scale)

Explanation:

Since the question asked about a range, the scale would be the most logical answer since scales are used to measure.

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_________.__________ and___________ are energy science

Artist 52 [7]

Answer:

Chemical, Mechanical, and Nuclear Energy

Explanation:

3 0

3 years ago

What mass of CO2 would be needed to weigh out to make 10.5 moles of carbon dioxide? (round answer to nearest tenth)

melamori03 [73]

The mass of carbon dioxide that would be needed to weigh is 462 grams.

Given:

10.5 moles of carbon dioxide.

The periodic table

To find:

The mass of carbon dioxide would be needed to weigh out to make 10.5 moles of carbon dioxide.

Solution:

Mass of carbon dioxide needed = m

Moles of carbon dioxide needed = 10.5 mol

The molar mass of carbon dioxide = M

The atomic mass of carbon atom = 12.011 g/mol

The atomic mass of oxygen atom = 15.999 g/mol

$M = 1\times 12.011 g/mol+2\times 15.999 g/mol\\\\=44.009 g/mol$

The moles of carbon dioxide will be given as:

$10.5 mol=\frac{m}{44.009 g/mol}\\\\m=10.5 mol\times 44.009 g/mol=462.0945 g\approx 462 g$

The mass of carbon dioxide that would be needed to weigh is 462 grams.

Learn more about the moles of substance here:

brainly.com/question/2293005?referrer=searchResults

brainly.com/question/1445383?referrer=searchResults

7 0

3 years ago

How many oxygen atoms are there in 3 molecules of CH3FO?

lbvjy [14]

Answer: There should be 3.

Explanation:

7 0

4 years ago

How much heat in joules is gained when a 34.5 g bar of gold is heated from 26.4°C to 75.3°C ?specific heat of gold on 0.129 J/gr

Sati [7]

Answer:

Q = 217.63J

Explanation:

Data;

Mass = 34.5g

T1 = 26.4°C

T2 = 75.3°C

c = 0.129J/g°C

Energy (Q) = mc(T2 - T1)

Q = 34.5 * 0.129 *(75.3 - 26.4)

Q = 4.4505 * 48.9

Q = 217.629J

Q = 217.63J

The heat gained was 217.63J

7 0

3 years ago

The normal freezing point of cyclohexane is 6.55 C. When 0.458 g of benzophenone is dissolved in 15.0 g of cyclohexane, the free

ella [17]

Answer:

The experimental molar mass of benzophenone is 182 g/m (option A)

Explanation:

ΔT = Kf . m . i

(i means the Van't Hoff factor, since benzophenone is not electrolyte, the value for i is 1)

ΔT = T° - T' (Melting temp sv pure - Melting temp sv in sl)

Kf is data (the cryoscopic constant)

m is molality (moles from solute in 1kg of solvent)

6,55°C - 3,19°C = 20,0° C/m . m

3,36 °C = 20,0 C/m . m

3,36 °C /20,0 m/C = m

0,168 = m

We have 0,168 moles of benzophenone in 1 kg of cyclohexane but we don't have 1kg, we have just 15 g so, we need the rule of three.

1000 g ______ 0,168 moles

15 g ________ (15 g . 0,168 m) / 1000 g = 0,00252 m

Now we can get the molar mass:

0,458 g of benzophenone / 0,00252 moles = 181,7 g/m

3 0

3 years ago