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Brrunno [24]
3 years ago
10

A student takes an object with an accepted mass of 120.0 grams and masses it on their

Chemistry
1 answer:
Varvara68 [4.7K]3 years ago
5 0

Answer:

<h2>The answer is 5.25 %</h2>

Explanation:

The percentage error of a certain measurement can be found by using the formula

P(\%) =  \frac{error}{actual \:  \: number}  \times 100\% \\

From the question

actual mass = 120 g

error = 120 - 113.7 = 6.3

The percentage error is

P (\%) =  \frac{6.3}{120}  \times 100 \\  = 5.25

We have the final answer as

<h3>5.25 %</h3>

Hope this helps you

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bagirrra123 [75]

Answer:

C3F7

'Tri' means 3

Tricarbon means 3 carbon

"Hepta" means 7

Fluoridez molecular formula is "F"

hence F7

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2 years ago
(1.8 x 10-2) ÷ (9 x 102) =
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A sample of gas occupies 3.00 L with 5.00 moles present. What would
pantera1 [17]

3/5 times 5/3x = 8*3/5. X=24/5 simplified would be x= 4.8 L.

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2 years ago
What state of matter has a definite shape and volume.
anastassius [24]

Solids have a definite shape and volume. They are always the same shape no matter what they are contained in; their volume is also the same because they don't change unless you add or take away from it.

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Liquids have an indefinite shape but definite volume. They expand to fill out the space they are contained in, but their volume doesn't change unless you take out or add more of the liquid.

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3 0
3 years ago
A sample of nitrogen gas is at a temperature of 50 c and a pressure of 2 atm. If the volume of the sample remains constant and t
Lilit [14]

Answer:

The new temperature of the nitrogen gas is 516.8 K or 243.8 C.

Explanation:

Gay-Lussac's law indicates that, as long as the volume of the container containing the gas is constant, as the temperature increases, the gas molecules move faster. Then the number of collisions with the walls increases, that is, the pressure increases. That is, the pressure of the gas is directly proportional to its temperature.

Gay-Lussac's law can be expressed mathematically as follows:

\frac{P}{T} =k

Where P = pressure, T = temperature, K = Constant

You want to study two different states, an initial state and a final state. You have a gas that is at a pressure P1 and at a temperature T1 at the beginning of the experiment. By varying the temperature to a new value T2, then the pressure will change to P2, and the following will be fulfilled:

\frac{P1}{T1} =\frac{P2}{T2}

In this case:

  • P1= 2 atm
  • T1= 50 C= 323 K (being 0 C= 273 K)
  • P2= 3.2 atm
  • T2= ?

Replacing:

\frac{2 atm}{323 K} =\frac{3.2 atm}{T2}

Solving:

T2*\frac{2 atm}{323 K} =3.2 atm

T2=3.2 atm*\frac{323 K}{2 atm}

T2= 516.8 K= 243.8 C

<u><em>The new temperature of the nitrogen gas is 516.8 K or 243.8 C.</em></u>

5 0
3 years ago
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