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2 years ago

What would happen if this cell were moved from pure water to a seawater solution?

1 answer:

3 0

<span>The cell would swell and burst, because the 20% salt solution is hypotonic with respect to the cell, causing a net movement of water into the cell. Example, water moves from the blood filtrate that will form urine. The same will do while pure water moved to seawater.</span>

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Which of the following would not be considered an observation in terms of the scientific method?

prohojiy [21]

Answer:

the first option, tasting a pasta sauce after adding a new ingredient.

Explanation:

tasting a pasta sauce after adding a new ingredient is not an observation because there is no qualitative or quantitative data to be taken from that experience.

4 0

2 years ago

I WILL GIVE BRAINLIEST TO WHOEVER ANSWERS FIRST

snow_tiger [21]

Answer:

I think it's B

Explanation:

I might be wrong, but please tell me.

5 0

2 years ago

2. How many moles are in 8.30 x 1023 molecules of H2O?

daser333 [38]

Answer:

<h2>1.38 moles</h2>

Explanation:

To find the number of moles in a substance given it's number of entities we use the formula

$n = \frac{N}{L} \\$

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

$n = \frac{8.30 \times {10}^{23} }{6.02 \times {10}^{23} } = \frac{8.30}{6.02} \\ = 1.3787 37...$

We have the final answer as

<h3>1.38 moles</h3>

Hope this helps you

8 0

2 years ago

A period of the periodic table ends with the highest energy level of an element's ators<br> having?"

andrey2020 [161]

Answer:

the last period. i think has the largest energy level

Explanation:

7 0

2 years ago

How many grams of XeF6 are required to react with 0.579 L of hydrogen gas at 4.46 atm and 45°C in the reaction shown below?

natka813 [3]

Answer:

8.1433 g of XeF₆ are required.

Explanation:

Balanced chemical equation;

XeF₆ (s) + 3H₂ (g) → Xe (g) + 6HF (g)

Given data:

Volume of hydrogen = 0.579 L

Pressure = 4.46 atm

Temperature = 45 °C (45+273= 318 k)

Solution:

First of all we will calculate the moles of hydrogen

PV = nRT

n = PV/ RT

n = 4.46 atm × 0.579 L / 0.0821 atm. dm³. mol⁻¹. K⁻¹ × 318 K

n = 2.6 atm . L / 26.12 atm. dm³. mol⁻¹

n = 0.0995 mol

Mass of hydrogen:

Mass = moles × molar mass

Mass = 0.0995 mol × 2.016 g/mol

Mass = 0.2006 g

Now we will compare the moles of hydrogen with XeF₆ from balance chemical equation.

H₂ : XeF₆

3 : 1

0.0995 : 1/3× 0.0995 = 0.0332 mol

Now we will calculate the mass of XeF₆.

Mass = moles × molar mass

Mass = 0.0332 mol × 245.28 g/mol

Mass = 8.1433 g

4 0

2 years ago