Describe the path of a carbon atom through the process of cellular respiration? PLEASE HELP!!!!

Answers

Answer 1

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You start with an equimolar mixture of the gases SO₂ and O₂ in a container. The SO₂ and O₂ react to completion to form SO₃. If the temperature after the reaction is 25°C and the pressure in the container is 1.65 atm, what is the density of the product gas mixture? Assume ideal behavior.

Answers

The density of the product gas mixture is 5.39 g/L

Explanation:

Given:

Temperature after the reaction = $25^0$ C

Pressure in the container = 1.65 atm

The ideal gas equation PV = nRT

To find: Density of the product gas mixture

Step 1:

Molarity (M) = P/(RT)

$\[M=(P)/(R T)\]$M=\frac{1.65 \mathrm{atm}}{\left(0.08206 (L \cdot a t m)/(m o l . K)\right)(298.15 K)}$$

M = 0.0674 mol/L

Step 2:

The product of the given reaction is $SO_3$ . Its molar mass is

1S x 32.066 g/mol = 32.066 g/mol

3O x 16 g/mol = 48 g/mol

Adding both we get 80.066 g/mol

Therefore the density of the product gas mixture is $0.0674 \frac{{mol}}{L} * \frac{80.066 g}{1 \mathrm{mol}}$

= 5.39 g/L

Before you touch a wire in an appliance how should you make sure that it is not energized

Answers

Answer:by checking for voltage with a neon tester

Explanation:

Hey There!

The device used to determine if there is energy in a wire is called a clamp meter, this device would detect if there are any presents currents in the wire. In order to use this device, you would simply have to attach it on the wire you are testing for.

Another device used to detect energy from wires is called a a non-contact voltage detector. While this device does not operate on all types of wires, it is solely created for AC circuits. Though, it is not preferred to manage the wire as this device sometimes proves to not be very reliable.

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10g of hyrogen react with excess of oxygen gas according to the equation:2H2+O2---->2H2O
what is the reacted volume of oxygen gas at STP and the mass of the produced water vapour in this reaction ?

Answers

Answer:

Volume of O₂ = 56 dm³

mass of water vapors (H₂O) = 90 g

Explanation:

Data Given:

mass of Oxygen = 10 g

Volume of Oxygen = ?

mass of the water vapor = ?

Reaction Given:

2H₂+O₂---->2H₂O

Solution:

First we have to look at the reaction for the information required

2H₂ + O₂ -------> 2H₂O

2 mol 1mol 2 mol

now convert moles to grams

molar mass of H₂ = 2(1) = 2 g/mol

molar mass of O₂ = 2(16) = 32 g/mol

molar mass of H₂0 = 2(1) + 16 = 18 g/mol

So the masses will be

2H₂ + O₂ -------> 2H₂O

2 mol (2 g/mol) 1mol (32 g/mol) 2 mol (18 g/mol)

4 g 32 g 36 g

So now we know that

4 g of hydrogen combine with 32 g of Oxygen and give 36 g of water vapors.

By using above information

First we find the volume of Oxygen:

For this first we find mass and then moles of Oxygen

As we know

if 4 g of hydrogen combine with 32 g of Oxygen then how much oxygen will react with 10 g of hydrogen

Apply unity formula

4 g of hydrogen H₂ ≅ 32 g of Oxygen O₂

10 g of hydrogen H₂ ≅ X g of Oxygen O₂

by doing Cross multiplication

g of Oxygen O₂ = 32 g x 10 g / 4 g

g of Oxygen O₂ = 80 g

So,

mass of oxygen = 80 g

now find moles of oxygen

formula used:

no. of moles = mass in grams/ molar mass . . . . . . (1)

Put values in above equation 1

no. of moles = 80 g / 32 g/mol

no. of moles = 2.5

Now to find volume of oxygen

Formula used

Volume of O₂ = no. of moles x molar volume (22.4 dm³/ mol) . . . . . . (2)

Put values in equation 2

Volume of O₂ = 2.5 moles x 22.4 dm³/mol

Volume of O₂ = 56 dm³

______________________

Now to find mass of water vapors

As we now

if 4 g of hydrogen produce 36 g of water vapors then how much water vapor will produce from 10 g of hydrogen

Apply unity formula

4 g of hydrogen H₂ ≅ 36 g of water vapors (H₂O)

10 g of hydrogen H₂ ≅ X g of water vapors (H₂O)

by doing Cross multiplication

g of water vapors (H₂O) = 36 g x 10 g / 4 g

g of water vapors (H₂O) = 90 g

So,

mass of water vapors (H₂O) = 90 g

N2 + 6e → 2N-3The reaction above represents which of the following?
a. Reduction
b. Decomposition
Oxidation
d. Acid-Base Netralization

Answers

Answer:

The correct answer is reduction.

Explanation:

Nitrogen gas reacts with hydrogen gas and get reduced to form ammonia. In this reaction.This is important reaction of atmospheric nitrogen fixation.The reaction is carried out by many nitrogen fixing bacteria such as Azotobacter,Clostridium etc.

N2+3H2+6e- = 2NH3

Final answer:

The reaction N2 + 6e → 2N-3 represents reduction, where nitrogen gains electrons to form N-3 ions.

Explanation:

The reaction N2 + 6e → 2N-3 represents reduction. In this reaction, nitrogen (N2) gains electrons (e) to form N-3 ions. Reduction is a process in which an atom or ion gains electrons, resulting in a decrease in its oxidation state.