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emmainna [20.7K]

3 years ago

10

Please Help and don't look it up please give a real answer please and thanks sooo much Why is photosynthesis an example of a che

mical reaction, and why is it classified as endothermic?

1 answer:

Mrac [35]3 years ago

3 0

Answer:

Photosynthesis is a chemical reaction

Explanation:

In which carbon dioxide (CO₂)and water (H₂O) are converted into glucose (C₆H₁₂O₆) and oxygen (O₂ ) with the help of chlorophyll and enzyme RuBisCO. It is classified as an endothermic reaction as it requires the input of energy in the form of solar energy.

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determine the empirical and molecular formula of a compound composed of 18.24 g carbon, 0.51 g hydrogen, and 16.91 g fluorine an

Vika [28.1K]

Answer: The empirical formula for the given compound is $C_3HF_2$ and molecular formula for the given compound is $C_{24}H_8F_{16}$

Explanation : Given,

Mass of C = 18.24 g

Mass of H = 0.51 g

Mass of F = 16.91 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{18.24g}{12g/mole}=1.52moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.51g}{1g/mole}=0.51moles$

Moles of Fluorine = $\frac{\text{Given mass of Fluorine}}{\text{Molar mass of Fluorine}}=\frac{16.91g}{19g/mole}=0.89moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.51 moles.

For Carbon = $\frac{1.52}{0.51}=2.98\approx 3$

For Hydrogen = $\frac{0.51}{0.51}=1$

For Fluorine = $\frac{0.89}{0.51}=1.74\approx 2$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : F = 3 : 1 : 2

The empirical formula for the given compound is $C_3H_1F_2=C_3HF_2$

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is :

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

We are given:

Molar mass = 562.0 g/mol

Mass of empirical formula = 3(12) + 1(1) + 2(19) = 75 g/eq

Putting values in above equation, we get:

$n=\frac{562.0}{75}=7.49\approx 8$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_3HF_2=(C_3HF_2)_n=(C_3HF_2)_8=C_{24}H_8F_{16}$

Thus, the molecular formula for the given compound is $C_{24}H_8F_{16}$

8 0

3 years ago

What is the volume of 1.9 moles of chlorine gas (Cl2) at 298 K and 1.3 atm?

matrenka [14]

<h2>Hello!</h2>

The answer is:

The correct option is option C.

$V=36L$

<h2>Why?</h2>

To calculate the volume of the gas sample, we need to use the Ideal Gas Law, this equation is used to relate the pressure, the volume, the mass and the temperature of a gas, so, we can isolate the volume from it.

The Ideal Gas Law equation is equal to:

$PV=nRT$

Where,

P is the pressure (in atm)

V is the volume (in liter)

n is the mass of the gass (in mole)

T is the temperature of the gass (absolute temperature)

So, from the statement we know that:

$Pressure=1.3atm\\Temperature=298K\\n=1.9moles\\R=0.082057\frac{L.atm}{mol.K}$

Then, substituting and calculating we have:

$PV=nRT\\\\V=\frac{nRT}{P}=\frac{1.9moles*0.082057\frac{L.atm}{mol.K}*298K}{1.3atm}=35.74L$

Now, rounding to the nearest whol number we have that the volume is equal to 36 L.

Hence, the correct option is option C.

Have a nice day!

5 0

3 years ago

Please answer ASAP I’ll give the brainliest!

lilavasa [31]

1. 1 mol=6.02.10²³ particles

$\tt \dfrac{3.63\times 10^{23}}{6.02\times 10^{23}}=0.602~moles$

2. Molar mass = Total atomic mass of component

AlBr₃ = Ar Al + 3. Ar Br

AlBr₃ = 27 + 3. 80 = 267 g/mol

3. mass = mol x MW

MW MnCl₂ = 55 + 2.35.5=126 g/mol

mass = 31.6 x 126 =3981.6 g

4. at STP, 1 mol =22.4 L, so for 5.6 L :

$\tt \dfrac{5.6}{22.4}=0.25~moles$

5. moles = mass : MW

MW CH₃OH = 12.1 + 4. 1 + 16.1 =32 g/mol

$\tt moles=\dfrac{0.5}{32}=0.016$

6. 1 mol = 22.4 L at STP

1 mol = 6.02.10²³ particles

moles for 8.20 x 10¹⁴ molecules

$\tt \dfrac{8.2\times 10^{14}}{6.02\times 10^{23}}=1.36\times 10^{-9}$

volume :

$\tt 1.36\times 10^{-19}\times 22.4=3.05\times 10^{-8}~L$

4 0

3 years ago

ANSWERRRRRRRRRRRRRRR PLEASEEEEEEEEEEEEEEEEEEEEEEEEEEEEEREEEEEEE

MAXImum [283]

Answer:

The 2nd choice correctly models a longitudinal wave. (I attached a pic)

Explanation:

It starts off compression and next is rarefaction. It then continues to go back and forth between the two.

Hope that helps!!

:D

4 0

3 years ago

How many moles of oxygen are needed to completely react with 9.5 g of sodium

maria [59]

<span>4 Na + O</span>₂<span> = 2 Na</span>₂<span>O
</span>
4* 23 g Na --------> 16 g O₂
9.5 g Na ------------> ?

Mass of O₂ = 9.5 * 16 / 4 * 23

Mass = 152 / 92

Mass = 1.6521 g of O₂

Molar mass O₂ = 16.0 g/mol

1 mole O₂ ------------ 16.0 g
? mole O₂ ------------ 1.6521 g

mole O₂ = 1.6521 * 1 / 16.0

≈ 0.10325 moles of O₂

hope this helps!

8 0

3 years ago