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Lisa [10]
2 years ago
7

What splits into carbon and oxygen atoms

Chemistry
1 answer:
OLga [1]2 years ago
8 0
When light breaks apart CO2, the molecule normally splits into carbon monoxide (CO) and an oxygen atom (O).
You might be interested in
What is the density of a sample of a substance with a volume of 120ml<br> and a mass of 90g?
tigry1 [53]

Answer:

<h3>The answer is 0.75 g/mL</h3>

Explanation:

The density of a substance can be found by using the formula

density =  \frac{mass}{volume}  \\

From the question

mass = 90 g

volume = 120 mL

We have

density =  \frac{90}{120}  =  \frac{9}{12}  =  \frac{3}{4}  \\

We have the final answer as

<h3>0.75 g/mL</h3>

Hope this helps you

6 0
2 years ago
NADH is also used by cells when making certain molecules. Based on your knowledge of the role of NADH in cellular respiration, w
OLEGan [10]

Answer:

Reducing molecules.

Explanation:

NAD (Nicotinamide adenine dinucleotide) is the important molecule used by the living organisms for the generation of ATP. NADH is used almost in every biochemical cycle like glycolysis, kreb cycle and elelctron transport chain.

The NADH molecule is used as the reducing molecule in the biosynthesis of the different reaction. The NADH molecule reduces its hydrogen ions and also carry electrons for the synthesis of molecules. The NADH molecule is also used in the shuttle system as well.

Thus, the answer is reducing molecules.

6 0
2 years ago
At standard ambient temperature and pressure (SATP), a gas has density of 1.5328g/L. What is the molar mass of the gas?
ahrayia [7]

The standard ambient temperature and pressure are

Temperature =298 K

Pressure = 1atm

The density of gas is 1.5328 g/L

density = mass of gas per unit volume

the ideal gas equation is

PV = nRT

P = pressure = 1 atm

V = volume

n = moles

R= gas constant = 0.0821 Latm/mol K

T = 298 K

moles = mass / molar mass

so we can write

n/V = density / molar mass

Putting values

Pressure=\frac{nRT}{V}=\frac{massXRT}{VXmolarmass}

Pressure=\frac{densityXRT}{molarmass}

molarmass=\frac{densityXRT}{Pressure}=\frac{1.5328X0.0821X298}{1}=37.50

Thus molar mass of gas is 37.50g/mol

6 0
3 years ago
What is the excess reactant in the combustion of 23 g of methane in the open atmosphere?
Marta_Voda [28]

Answer : The excess reactant in the combustion of methane in opem atmosphere is O_{2} molecule.

Solution : Given,

Mass of methane = 23 g

Molar mass of methane = 16.04 g/mole

The Net balanced chemical reaction for combustion of methane is,

CH_4(g)+2O_2(g)\rightarrow CO_2(g)+2H_2O(g)

First we have to calculate the moles of methane.

\text{ Moles of methane}=\frac{\text{ Given mass of methane}}{\text{ Molar mass of methane}} = \frac{23g}{16.04g/mole} = 1.434 moles

From the above chemical reaction, we conclude that

1 mole of methane react with the 2 moles of oxygen

and 1.434 moles of methane react to give \frac{2moles\times 1.434moles}{1moles} moles of oxygen

The Moles of oxygen = 2.868 moles

Now we conclude that the moles of oxygen are more than the moles of methane.

Therefore, the excess reactant in the combustion of methane in open atmosphere is O_{2} molecule.


6 0
3 years ago
Question 25 of 33
Dafna11 [192]

Answer:

A) It tends to increase from top to bottom of a group

6 0
2 years ago
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