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tekilochka [14]

2 years ago

9

⦁ How many moles of carbon dioxide will be produced by the complete reaction of 2.0 mol of glucose (C6H12O6), according to the f

ollowing equation?
C6H12O6 + 6O2 → 6CO2 + 6H2O

1 answer:

SashulF [63]2 years ago

3 0

Answer:

i think 12 moles of CO2 will be produced

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A light source of wavelength, l, illuminates a metal and ejects photoelectrons with a maximum kinetic energy of 1 eV. A second l

madreJ [45]

Explanation:

From first source, kinetic energy ( $K.E_{1}$ ) ejected is 1 eV and wavelength of light is $\lambda$ .

From second source, kinetic energy ( $K.E_{2}$ ) ejected is 4 eV and wavelength of light is $\frac{\lambda}{2}$ .

Relation between work function, wavelength, and kinetic energy is as follows.

K.E = $\frac{hc}{\lambda} - \phi$

where, h = Plank's constant = $6.63 \times 10^{-34}$ J.s

c = speed of light = $3 \times 10^{8}$ m/s

Also, it is known that 1 eV = $1.6 \times 10^{-19}$ J

Therefore, substituting the values in the above formula as follows.

From first source,

$K.E_{1}$ = $\frac{hc}{\lambda} - \phi$

1 eV = $1.6 \times 10^{-19} J = \frac{6.63 \times 10^{-34} \times 3 \times 10^{8}}{\lambda} - \phi$

$1.6 \times 10^{-19} J = \frac{1.98 \times 10^{-25} J.m}{\lambda} - \phi$ ........... (1)

From second source,

$K.E_{2}$ = $\frac{hc}{\lambda} - \phi$

$4 \times 1.6 \times 10^{-19} J = \frac{6.63 \times 10^{-34} \times 3 \times 10^{8}}{\frac{\lambda}{2}} - \phi$

$6.4 \times 10^{-19} J = \frac{2 \times 1.98 \times 10^{-25} J.m}{\lambda} - \phi$ ........... (2)

Now, divide equation (2) by 2. Therefore, it will become

${6.4 \times 10^{-19}J}{2} = \frac{2 \times 1.98 \times 10^{-25} J.m}{2\lambda} - \frac{\phi}{2}$

$3.2 \times 10^{-19}J = \frac{1.98 \times 10^{-25} J.m}{\lambda} - \frac{\phi}{2}$ ......... (3)

Now, subtract equation (3) from equation (1), we get the following.

$1.6 \times 10^{-19} = \frac{\phi}{2}$

$\phi$ = $3.2 \times 10^{-19}$

= 2 eV

Thus, we can conclude that work function of the metal is 2 eV.

3 0

3 years ago

How many grams of O2 are produced as 0.033 mol of water decompose

PolarNik [594]

Answer: This can be quickly solved with "traintracks"

Explanation:

You start w/ grams of water and want to find moles of oxygen gas produced.

So you want to Convert:

Grams of water -> moles of water -> moles of oxygen gas.

The two things you need to know to set up the tracks are:

1)Molar mass of water- H2O

Hydrogen - 1.008(x2)

Oxygen - 16.00

Water - 18.016

6 0

3 years ago

How many valence electrons does Oxygen have:<br> a) 3 <br> b) 5 <br> c) 13

ivolga24 [154]

Answer:

it has 6?

Explanation:

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2 years ago

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What charge would you expect for an formed by P?

Alex73 [517]

Answer:

friend according to the question the answer is +3 ....

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2 years ago

How many grams of CO2 are used when 7 g of oxygen are produced

lara [203]

308 grams of co2 is used

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2 years ago