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Nina [5.8K]
2 years ago
6

Question 2 (Multiple Choice Worth 2 points)

Chemistry
1 answer:
faust18 [17]2 years ago
6 0

Answer:

\pi r²  x h

Explanation:

A can is cylindrical in nature. Using the formula of the volume of the can, we can find this unknown volume.

The volume of cylinder is given as:

   Volume of a cylinder  = Area x height

  Volume of  a cylinder = \pi r²  x h

Therefore density of the can;

      Density  = \frac{mass}{volume}

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A great white shark has resided at a depth where the pressure is 16 atm. If the initial volume of its swim bladder is 4 L, what
padilas [110]

Answer:

The new volume of the gas is 32L

Explanation:

P1 = 16atm

V1 = 4L

P2 = atm

V2 = ?

According to Boyle's law, the volume of a given mass of gas is inversely proportional to its volume provided the temperature remains constant.

P1 * V1 = P2 * V2

V2 = (P1 * V1) / P2

V2 = (16 * 4) / 2

V2 = 64 / 2

V2 = 32L

The new volume of the gas is 32L

6 0
3 years ago
An experiment shows that a 236 mL gas sample has a mass of 0.443 g at a pressure of 740 mmHg and a temperature of 22 ∘C. What is
aleksley [76]

Answer:

49.2 g/mol

Explanation:

Let's first take account of what we have and convert them into the correct units.

Volume= 236 mL x (\frac{1 L}{1000 mL}) = .236 L

Pressure= 740 mm Hg x (\frac{1 atm}{760 mm Hg})= 0.97 atm

Temperature= 22C + 273= 295 K

mass= 0.443 g

Molar mass is in grams per mole, or MM= \frac{mass}{moles} or MM= \frac{m}{n}. They're all the same.

We have mass (0.443 g) we just need moles. We can find moles with the ideal gas constant PV=nRT. We want to solve for n, so we'll rearrange it to be

n=\frac{PV}{RT}, where R (constant)= 0.082 L atm mol-1 K-1

Let's plug in what we know.

n=\frac{(0.97 atm)(0.236 L)}{(0.082)(295K)}

n= 0.009 mol

Let's look back at MM= \frac{m}{n} and plug in what we know.

MM= \frac{0.443 g}{0.009 mol}

MM= 49.2 g/mol

3 0
2 years ago
In a common laboratory experiment in general chemistry students are asked to determine:_____.
Alex787 [66]
<h3>The <u>complete question</u> would be:</h3>

In a common laboratory experiment in general chemistry, students are asked to determine the relative amounts of benzoic acid and charcoal in a solid mixture. Benzoic acid is relatively soluble in hot water, but charcoal is not. Devise a method for separating the two components in the mixture.

<h3>The <u>solution</u> for that would be:</h3>

First you put the mixture in hot water and allow the benzoic acid to separate. Next funnel it and then see what's on the funnel paper. Lastly, heat the leftover water and see what's left after it evaporates.

<h3><u>What are laboratory experiments ?</u></h3>
  • Using controlled surroundings to test theories, researchers may develop laboratory experiments.
  • Laboratories are rooms or specially constructed facilities within buildings that are often found on college and university campuses and are utilized for academic research.
  • It's crucial to differentiate between experiments and other kinds of research investigations carried out in lab settings.
  • Even if a research study takes place in a lab, it is not always an experiment.
  • In order to evaluate causal conclusions regarding the links between independent and dependent variables, laboratory studies, like all genuine experimental designs, use procedures of random assignment of participants and control groups.

To view more about experiments, refer to:

brainly.com/question/17143317

#SPJ4

3 0
10 months ago
How can you tell that a precipitate has formed?
ladessa [460]

Answer:

if a solid appears when mixing two liquids

Explanation:

i remember this question :D

7 0
3 years ago
Read 2 more answers
A sample of helium gas inside a closed but flexible container occupies a volume of 355mL at 23°C. If the pressure is held consta
guapka [62]

Answer:

978.19° C

Explanation:

P1V1/T1 =P2V2/T2     Since the pressure is constant, this can be written as

V1/T1 = V2/T2      RE-ARRANGE TO

V2 *  T1/V1   = T2       Note:  T must be in Kelvin!!

1.5 L  *  (273.15 + 23)  / (.355 L ) = T2 = 1251.338 K  =978.19 C

6 0
1 year ago
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