73 m is equal to how many dm?

The pressure caused by a sample of gas is 2.25 atm. 1 atm is

nexus9112 [7]

Answer:

$0.326\frac{N}{cm^2}$

Explanation:

Hello.

In this case, considering that 1 atm equals 1.01 kPa, we can compute the pressure in kPa first as shown below:

$2.25atm*\frac{1.01kPa}{1atm} =3.26kPa$

Now, we convert kPa to Pa, considering 1 kPa equals 1000 Pa:

$3.26kPa*\frac{1000Pa}{1kPa}=3260Pa$

Now, since Pa is equal to N/m², and 1 m equals 100 cm, the pressure in newton per square centimeter turns out:

$3260\frac{N}{m^2}*(\frac{1m}{100cm})^2 \\\\0.326\frac{N}{cm^2}$

Best regards.

4 0

3 years ago

What is the periodic table a list of

barxatty [35]

Answer:

i think c should be ur answer

5 0

2 years ago

Identify a type of strong intermolecular force that exists between water molecules, but does not exist between carbon dioxide mo

timurjin [86]

Intermolecular forces of attraction hold the molecules together. These forces determine the physical properties of substances like melting and boiling points. There are five types of intermolecular forces: Hydrogen bonding, dipole-dipole interactions, ionic interactions, ion-dipole interactions and dispersion forces.

Hydrogen bonding is a stronger force of attraction between hydrogen atom and an electronegative atom (F, N, and O). So, water molecules exhibit hydrogen bonding.

In carbon dioxide molecules, although each C=O is polar the molecule as a whole will be non polar due to symmetry. Therefore, the only intermolecular forces in CO2 will be dispersion forces.

Hence, Hydrogen bonding exists between water molecules but not carbon dioxide molecules.

7 0

3 years ago

Suppose of ammonium nitrate is dissolved in of a aqueous solution of sodium chromate. Calculate the final molarity of ammonium c

Marta_Voda [28]

Answer:

Final molarity of ammonium cation in the solution = 0.16 M

Explanation:

Complete Question

Suppose 2.59 g of ammonium nitrate is dissolved in 200. mL of a 0.40M aqueous solution of sodium chromate. Calculate the final molarity of ammonium cation in the solution. You can assume the volume of the solution doesn't change when the ammonium nitrate is dissolved in it. Be sure your answer has the correct number of significant digits.

Solution

2NH₄NO₃ + Na₂CrO₄ → (NH₄)₂CrO₄ + 2NaNO₃

We first convert the given parameters to number of moles

Number of moles = (Mass/Molar mass)

Molar mass of NH₄NO₃ = 80.043 g/mol

Number of moles of NH₄NO₃ = (2.59/80.043) = 0.03224 mole

Number of moles = (Concentration in mol/L) × (Volume in L)

Number of moles of Na₂CrO₄ = 0.4 × 0.2 = 0.08 Mole

2 moles of NH₄NO₃ react with 1 mole of Na₂CrO₄

So, it it evident that NH₄NO₃ is the limiting reagent as it is in short supply in the amount needed for the reaction.

So, the number of moles of ammonium ion in the product is also 0.03224 mole.

Molarity = (Number of moles)/(Volume L)

Molarity of ammonium ion = (0.03224/0.2) = 0.1612 mol/L = 0.16 M

Hope this Helps!!!

3 0

2 years ago

Which bonds are found inside a water molecule, between hydrogen and oxygen?

Papessa [141]

Hydrogen bond is found between water molecule if im correct

5 0

3 years ago