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3 years ago

What process in the carbon cycle takes carbon out of air?

1 answer:

7 0

It is photosynthesis

photosynthesis is the process by which green plants and some other organisms use sunlight to synthesize foods from carbon dioxide and water. photosynthesis in plants generally involves the green pigment chlorophyll and generates oxygen as a byproduct, hope it helps

You might be interested in

how does the processes of photosynthesis and cellular respiration allow for the flow of energy in organisms

Naddika [18.5K]

Photosynthesis and cellular respiration go hand and hand. Remember the two equations are just a reverse of the opposite equation.

Cellular Respiration-
C₆H₁₂O₆ + 6O₂ (Yeilds or Makes) 6CO₂ + 6H₂O + ATP (Or Energy)

Photosynthesis-
6CO₂ + 6H₂O + ATP (Or Sunlight) (Yeilds or Makes) C₆H₁₂O₆ + 6O₂

When a plant goes through photosynthesis it produces oxygen as a waste product, which you should know is what animals use to breathe, well when animals use oxygen in the process, they also make a waste product which happens to be Carbon Dioxide, which a plant uses to make glucose during photosynthesis, so if we didin't have one we wouldn't have the other.

8 0

3 years ago

Which is a binary compound?

nirvana33 [79]

Answer:

it is made up of two or more element

5 0

3 years ago

A sample of g of pure aluminum metal is added to mL of M hydrochloric acid. The volume of hydrogen gas produced at standard temp

MArishka [77]

Answer:

V = 11.2L are produced

Explanation:

... Sample of 27g of pure aluminium, 3added to 333 mL of 3.0 M HCl..

Based on the chemical reaction:

2Al(s) + 6HCl(aq) → 2AlC₃(aq) + 3H₂(g)

Where 3 moles of hydrogen are produced when 6 moles of hydrochloric acid reacts with 2 moles of Al.

To solve this question, we need to determine limiting reactant converting each reactant to moles. With limiting reactant and the chemical reaction we can find moles of hydrogen and its volume at STP (T=273.15K; P=1atm), thus:

Moles Al-Molar mass: 26.98g/mol-:

27g * (1mol / 26.98g) = 1mol of Al

Moles HCl:

333mL = 0.333L * (3mol/L) = 1mol HCl

For a complete reaction of 1 mole of HCl are required:

1mol HCl * (2mol Al / 6mol HCl) = 0.333 moles of Al. As there is 1 mole of Al, Al is in excess and HCl is limiting reactant.

Moles of Hydrogen produced are:

1mol HCl * (3 moles H₂ / 6 mol HCl) = 0.5moles H₂ are produced.

Using ideal gas law:

PV = nRT

V = nRT/P

Where V is volume

n are moles: 0.5mol

R is gas constant: 0.082atmL/molK

T is absolute temperature: 273.15K

P is pressure: 1atm.

Solving for V:

V = 0.5mol*0.082atmL/molK*273.15K / 1atm

<h3>V = 11.2L are produced</h3>

3 0

3 years ago

Calculate the energy for the transition of an electron from the n = 5 level to the n = 6 level of a hydrogen atom. E = Joules Is

kramer

Answer:

For an electron to move from a lower energy level to a higher energy , that electron needs to absorb energy sufficient enough to excite it to make the transition. Hence it is an absorption process. The required energy of transition E = 2.665 x 10⁻²⁰J

Explanation:

Using the Rydberg's equation we can calculate the wavelength of the photon of energy transition as follows:

1/λ = R . (1/nf² - 1/ni²)

where

λ is the required wavelength of the photon needed to be absorbed to excite the electron to transit from level 5 to 6.

(Note that for the electron to transit to from energy level 5 to 6, the photon would have to fall from level 6 to 5 in order to emit the required energy to excite the electron)

R is the Rydberg's constant 1.097 x 10⁷ m⁻¹

nf is the final level of the photon

ni is the initial level of the photon

1/λ = 1.097 x 10⁷ m⁻¹ (1/5² - 1/6²)

1/λ = 1.3407 x 10⁵ m⁻¹

λ = 7.458 x 10⁻⁶ m

This implies that that is the wavelength of the photon required to excite the electron to transit from energy level 5 to 6. Using the equation below, we can calculate the energy of transition as

E = h.c/λ

where

E is the required energy of transition

h is the Planck's constant (6.626 x 10⁻³⁴ Js)

c is the speed of light (3 x 10⁸ms⁻¹)

λ is the wavelength calculated above

E = 6.626 x 10⁻³⁴ Js x 3 x 10⁸ms⁻¹/ 7.458 x 10⁻⁶ m

E = 2.665 x 10⁻²⁰J

3 0

3 years ago

In the reaction 2H2O (l) + 2Cl– (aq) → H2 (g) + Cl2 (g) + 2OH– (aq), how many electrons are transferred?

lora16 [44]

C. 2

2H_2O + 2e^(-) → H_2 + 2OH^(-)

2Cl^(-) → Cl_2 + 2e^(-)

2H_2O +Cl^(-) + 2e^(-) → H_2 + Cl_2 + 2OH^(-) + 2e^(-)

2H_2O +2Cl^(-) → H_2 + Cl_2 + 2OH^(-)

This is a redox reaction in which two chloride ions transfer two electrons to two molecules of water.

7 0

3 years ago