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PolarNik [594]
3 years ago
6

(Please answer both, i'm giving 20 points) The more directly the sun strikes a place on earth’s surface, the more _______ the en

ergy is and the _______ it will be. Areas that receive less direct sunlight experience colder months.
Question 1 options:

less, colder


warmer, concentrated


colder, less


concentrated, warmer

Question 2 (0.5 points)
In the Northern Hemisphere, choose ALL that apply

Question 2 options:

Summer solstice occurs when the Earth's North Pole is tilted toward the sun.


Fall and Spring Equinoxes occur when days and nights are equal in length.


The tilt and revolution of the Earth causes the seasons


Winter solstice occurs when the Earth's North Pole is tilted away from the sun.
Chemistry
2 answers:
tekilochka [14]3 years ago
7 0

Answer:

The top one is b i need the 2nd 1

Explanation:

CaHeK987 [17]3 years ago
7 0

Answer:

Question 1

concentrated, warmer

Question 2

Is all of them

Explanation:

I took the test and got 100%

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In the laboratory, hydrogen gas is usually made by the following reaction: Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) How many liters
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<u>Answer:</u> The volume of hydrogen gas collected over water is 2.13 L

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass of zinc = 5.566 g

Molar mass of zinc = 65.4 g/mol

Putting values in above equation, we get:

\text{Moles of zinc}=\frac{5.566g}{65.4g/mol}=0.0851mol

For the given chemical reaction:

Zn(s)+2HCl(aq.)\rightarrow H_2(g)+ZnCl_2(aq.)

As, HCl is present in excess. So, it is considered as an excess reagent.

Zinc is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of zinc produces 1 mole of hydrogen gas.

So, 0.0851 moles of zinc will produce = \frac{1}[1}\times 0.0851=0.0851mol of hydrogen gas

To calculate the volume of hydrogen gas, we use ideal gas equation, which is:

PV = nRT

where,

P = Pressure of hydrogen gas = Total atmospheric pressure - vapor pressure of water = (752 - 18.65) mmHg = 733.35 mmHg

V = Volume of the hydrogen gas

n = number of moles of gas = 0.0851 moles

R = Gas constant = 62.3637\text{ L.mmHg }mol^{-1}K^{-1}

T = Temperature of hydrogen gas = 21^oC=[21+273]K=294K

Putting values in above equation, we get:

733.35mmHg\times V=0.0851mol\times 62.3637\text{ L.mmHg }mol^{-1}K^{-1}\times 294K\\\\V=\frac{0.0851\times 62.3637\times 294}{733.35}=2.13L

Hence, the volume of hydrogen gas collected over water is 2.13 L

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