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3 years ago

What energy convertion happens when green plants use energy from the sun to make sugar?

2 answers:

8 0

The energy conversion happening here is known as photosynthesis. Photosynthesis is a process where the leaves of a plant absorb water and carbon dioxide, then, using light energy from the sun, convert that into oxygen and sugar.

defon3 years ago

6 0

Answer:

Photosynthesis is the process plants use to convert energy from the sun into usable energy for their cells. Plants use the light energy of the sun, carbon dioxide, and water to make glucose (a sugar), and oxygen. The energy of the sun is captured and stored in the bonds between atoms in glucose molecules.

Explanation:

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Calculate the number of atoms in a 3.96 × 103 g sample of silicon.

Crank

Atomic mass Si = 28.0855 u.m.a

28.0855 g -------------------- 6.02x10²³ atoms
3.96x10³ g ------------------- ?? atoms

( 3.96x10³) x 6.02x10²³ / 28.0855 =

8.48x10²⁵ atoms

6 0

3 years ago

A space shuttle is used for space------

Gre4nikov [31]

Answer: YES THATS TRUE

Explanation:

8 0

3 years ago

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Considering the activity series given below for metals and nonmetals, which reaction will occur?

kozerog [31]

Answer:

the answer is C i just took the test

Explanation:

2AgNO3 + Ni Right arrow. Ni(NO3)2 + 2Ag

5 0

4 years ago

In a calorimeter, a 1.0 g sample of magnesium is burned to form mgo. in doing so, 25.5 kj of energy are released. what is the mo

Artemon [7]

The molar enthalpy of combustion in kj/mol of magnesium is 620 kj/mol, Option D is the correct answer.

<h3>What is enthalpy of Combustion ?</h3>

The energy released when a fuel is oxidized by an oxidizing agent is called enthalpy of Combustion.

It is given that

a 1.0 g sample of magnesium is burned to form MgO. in doing so, 25.5 kj of energy are released.

Molecular weight of Magnesium = 24.35g

24.35 g makes 1 mole of Mg

1g = 1/24.35

For 0.04 moles 25.5 kJ is released

for 1 mole 25.5 *1/.04

= 620 kj/mol

Therefore the molar enthalpy of combustion in kj/mol of magnesium is 620 kj/mol.

To know more about enthalpy of combustion

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3 0

2 years ago

A 0.590 gram sample of a metal, M, reacts completely with sulfuric acid according to:

Naddik [55]

Answer:

Molar mass of the metal = 59.0 g/mol

Explanation:

Vapor pressure of water at $25^oC$ = 23.78 torr

We are given:

Total vapor pressure = 756.0 torr

Vapor pressure of hydrogen gas = Total vapor pressure - Vapor pressure of water = (756.0 - 23.78) torr = 732.22 torr

To calculate the amount of hydrogen gas collected, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = 732.22 torr

V = Volume of the gas = 255 mL = 0.255 L ( 1 mL = 0.001 L )

T = Temperature of the gas = $25^oC=[25+273]K=298K$

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

n = number of moles of hydrogen gas = ?

Putting values in above equation, we get:

$732.22 torr\times 0.255L=n\times 62.3637\text{ L.torr }mol^{-1}K^{-1}\times 298K\\\\n=\frac{732.22\times 0.255}{62.3637\times 298}=0.01mol$

From the reaction shown below:-

$M+H_2SO_4\rightarrow MSO_4+H_2$

1 mole of hydrogen gas is produced when 1 mole of the metal is reacted.

Also,

0.01 mole of hydrogen gas is produced when 0.01 mole of the metal is reacted.

Moles of the metal = 0.01 mol

Mass taken = 0.590 g

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$0.01\ mole= \frac{0.590\ g}{Molar\ mass}$

Molar mass of the metal = 59.0 g/mol

5 0

4 years ago

Read 2 more answers