Balance the following chemical equation by providing the correct coefficients.

If each of the following compounds/ions were placed between 2 electrically charged plates (one positive and one negative) Which

GREYUIT [131]

<span>If a molecule wants to interact with an electric field. it should have a permanent dipole momentum. so first check the polarity. for example CH4 is not polar. CH2Cl2 is polar (so yes), H3O)+ is obvious that is polar. H2O yes. C2H2Cl2 in trans form is not polar but in cis form yes. CO2 is non-polar. Ozone is polar. </span>

4 0

2 years ago

Which of the following is not an example of a molecule?

dybincka [34]

Answer:

He

Explanation:

A molecule is the smallest physical unit of a substance that can exist independently, consisting of 2 or more atoms chemically combined

He is one atom of Helium

4 0

3 years ago

What volume does 2.25g of nitrogen gas, N2, occupy at 273 Celsius and 1.02 atm

kotykmax [81]

<h2><u>Answer:</u></h2>

0.126 Liters

<h2><u>Explanation:</u></h2>

V = mRT / mmP

First, convert the 2.25g of Nitrogen gas into moles. (m in the equation above)

2.25g x 1 mole / 28.0g = 0.08036 moles = m

28.0g = mm

Next, convert the 273 Celsius into Kelvin. (T in the equation above)

273 Celsius + 273.15 = 546.15K = T

R = 0.08206L*atm/mol*K

(Quick Note: The R changes depending on the Pressure Unit so do not use this number every time.)

Now, plug everything into the equation.

V = (0.08036)(0.08206)(546.15)/(28.0)(1.02)

V = 0.126 L

5 0

3 years ago

When the molecules of a gas hit each other do they normally stick or bounce off

Dahasolnce [82]

Since the molecules of a gas are constantly in motion, moving and hitting other gas molecules in all directions of the enclosed container, the molecules transfer a portion of energy through the interaction of other gas particles as they hit, but then bounce off.

8 0

2 years ago

Read 2 more answers

A 2.00-mol sample of hydrogen gas is heated at constant pressure from 294 K to 414 K. (a) Calculate the energy transferred to th

Furkat [3]

Answer:

a) The energy transferred is 6.91 kJ

b) The internal energy is 4.90 kJ

c) The work done on the gas is - 2.01 kJ

Explanation:

Step 1: Data given

Number of moles of hydrogen gas = 2.00 moles

Pressure = constant

Temperature is heated from 294 K to 414 K

Molar heat capacity of hydrogen gas = 28.8 J/mol*K

Step 2: Calculate the energy transferred to the gas by heat.

Q = n* Cp * ΔT

⇒with Q =the energy transferred

⇒with n = the number of moles = 2.00 moles

⇒with Cp = the Molar heat capacity of hydrogen gas = 28.8 J/mol*K

⇒ with ΔT = Temperature 2 - Temperature 1 = 414 - 294 = 120K

Q = 2.00 * 28.8 * 120

Q = 6912 J = 6.91 kJ

Step 3: Calculate the increase in its internal energy.

ΔEint = n*Cv*ΔT

⇒with ΔEint = the increase in its internal energy.

⇒with n = the number of moles = 2.00 moles

⇒with Cv = The constant volume = 20.4 J/mol*K

⇒with ΔT = Temperature 2 - Temperature 1 = 414 - 294 = 120K

ΔEint = 2.00 * 20.4 * 120

ΔEint =4896 J = 4.90 kJ

Step 4: Calculate the work done on the gas.

Work done on the gas = -Q + ΔEint

W = -6.91 kJ + 4.90 kJ

W = -2.01 kJ

6 0

3 years ago