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2 years ago

I've been waiting for like 10 mins. Please answer this.

Chemistry

2 answers:

Monica [59]2 years ago

8 0

the correct answer is B

Degger [83]2 years ago

3 0

The answer is B. 6CO2+H2O yields C6H12O6+ 6H20.

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Assume that the pressure inside of the 1 liter balloon is 200,000 Pa, what is the explosive energy in the inside the balloon? Ex

AysviL [449]

Answer:

200 Joules is the explosive energy in the inside the balloon. And that is $9.523\times 10^{-5}$ 1 lb of TNT.

Explanation:

$Pressure=\frac{force}{Area}=\frac{Force\times distance}{Area \times distance}=\frac{Energy}{Volume}$

Volume of the balloon = V = 1 L = $0.001 m^3$

Pressure inside the balloon ,P= 200,000 Pa = $200,000 N/m^2$

Explosive energy in the inside the balloon be E.

E = Pressure × Volume

$E=200,000 N/m^2\times 0.001 m^3=200 Joules$

1 lb of TNT = $2.1\times 10^6 J$

200 Joules = $200\times \frac{1}{2.1\times 10^6 }$ 1 lb of TNT

= $9.523\times 10^{-5}$ 1 lb of TNT

5 0

3 years ago

What is an ion? Describe and give an example.

Goshia [24]

An ion is a charged atom or molecule. It is charged because the number of electrons do not equal the number of protons in the atom or molecule. An atom can acquire a positive charge or a negative charge depending on whether the number of electrons in an atom is greater or less then the number of protons in the atom. An example is Iron (III) , Iron (II) , lithium, and hydrogen.

3 0

2 years ago

Read 2 more answers

Does acid rain make new substances?

ivanzaharov [21]

Answer:

Over the past few decades, humans have released so many different chemicals into the air that they have changed the mix of gases in the atmosphere. ... In addition, the exhaust from cars, trucks, and buses releases nitrogen oxides and sulfur dioxide into the air.

3 0

2 years ago

Chlorine pentafluoride gas is collected at -17.0 °C in an evacuated flask with measured volume of 35.0 L. When all the gas has b

Svet_ta [14]

Answer:

1. The mass of Chlorine pentafluoride, ClF5, is 39.16g

2. The number of mole of Chlorine pentafluoride, ClF5, is 0.3mole

Explanation:

1. To solve the mass of Chlorine pentafluoride, ClF5, first, let us calculate the molar mass of ClF5. This is illustrated below:

Molar Mass of ClF5 = 35.5 + (5 x 19) = 35.5 + 95 = 130.5g/mol

From the ideal gas equation:

PV = nRT (1)

Recall:

Number of mole(n) = mass (m) /Molar Mass(M)

n = m/M

Now substituting the value of n in equation 1, we have:

PV = nRT

PV = mRT/M

Now we can obtain the mass of Chlorine pentafluoride ClF5 as follow:

Data obtained from the question include:

T (temperature) = -17.0 °C = - 17 + 273 = 256K

V (volume) = 35L

P (pressure) = 0.180 atm

R (gas constant) = 0.082atm.L/Kmol

m (mass of Chlorine pentafluoride) =?

M (molar mass of Chlorine pentafluoride) = 130.5g/mol

PV = mRT/M

0.180 x 35 = m x 0.082 x 256/ 130.5

Cross multiply to express in linear form as shown below:

m x 0.082 x 256 = 0.180x35x130.5

Divide both side by 0.082 x 256

m = (0.180x35x130.5) /(0.082x256)

m = 39.16g

Therefore, the mass of Chlorine pentafluoride, ClF5, is 39.16g

2. The number of mole of ClF5 can be obtained as follow:

Mass of ClF5 = 39.16g

Molar Mass of ClF5 = 130.5g/mol

Mole of ClF5 =?

Number of mole = Mass /Molar Mass

Mole of ClF5 = 39.16/130.5g

Mole of ClF5 = 0.3mole

8 0

3 years ago

Read 2 more answers

A sample of krypton gas with a volume of 10.00 L has a temp of 303 K and exerts

marshall27 [118]

<u>Answer:</u> The final volume will be 14.85 L.

<u>Explanation:</u>

To calculate the final volume when temperature increases, we use Charles' Law.

This law states that volume is directly proportional to the temperature of the gas if number of moles and pressure remains constant.

$V\propto T\\\\\frac{V_1}{T_1}=\frac{V_2}{T_2}$

where,

$V_1\text{ and }T_1$ = Initial volume and temperature

$V_2\text{ and }T_2$ = Final volume and temperature

We are given:

$V_1=10L\\
T_1=303K\\
V_2=?L\\
T_2=450K$

Putting values in above equation, we get:

$\frac{10L}{303K}=\frac{V_2}{450K}$

$V_2=14.85L$

Hence, the final volume of the gas is 14.85L

7 0

3 years ago