All categories

3 years ago

The average kinetic energy of water molecules is greatest in which of these samples?

Chemistry

1 answer:

shutvik [7]3 years ago

7 0

Your answer will be

B- 10g of water at 55 c

Sorry i cant find the Fahrenheit on my friend computer

You might be interested in

Place the following in order of increasing IE1

lyudmila [28]

Answer:

A) As < N < F

Explanation:

Ionization energy refers to the minimum amount of energy required to remove an electron from a gaseous atom r in.

The genera trend of IE, is that it increases across the period from left to right and decrease down the group in a periodic table.

As belongs to period 4, this means it as the lowest ionization energy.

Nitrogen and Florine belong to the same period however Florine has a higher ionization energy.

In order of increasing IE;

As < N < F

7 0

3 years ago

A sample of gas has a volume of 2.4 L and a pressure of 1.2 atm. What would the pressure of the same gas sample be if the volume

algol [13]

Answer:

The correct answer option is 1.6 atm.

Explanation:

We know that there is a sample gas which has a volume of 2.4 L with a pressure 1.2 atm and we are to find the pressure of the same gas sample if its volume is reduced to 1.8 L at a constant temperature.

We will apply the Boyle's law here which states that the "pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature".

$P_1V_1=P_2V_2$

Substituting the values in the formula to get:

$P_2=\frac{1.2*2.4}{1.8} \\\\P_2=1.6$

Therefore, the pressure of the same gas sample will be 1.6 atm if the volume is reduced to 1.8 L at a constant temperature.

3 0

3 years ago

What is the partial pressure of helium gas in a mixture that contains 8.00 grams of helium and 8.60 mol argon gas with a total p

Agata [3.3K]

Answer:

$P_{He}=9.06torr$

Explanation:

Hello there!

In this case, we can identify the solution to this problem via the Dalton's rule because the partial pressure of helium is given by:

$P_{He}=x_{He}P_T$

Whereas the mole fraction of helium is calculated by firstly obtaining the moles and then the mole fraction:

$n_{He}=8.00g\frac{1mol}{4.00g}=2.00mol\\\\ x_{He}=\frac{n_{He}}{n_{He}+n_{Ar}} \\\\ x_{He}=\frac{2.00mol}{2.00mol+8.60mol}\\\\x_{He}=0.189$

Then, we calculate the partial pressure as shown below:

$P_{He}=0.189 *48.0torr\\\\P_{He}=9.06torr$

Best regards!

4 0

3 years ago

Calculate the percent of composition of oxygen in Mercury (ll) oxide HgO

bekas [8.4K]

Add up the molar mass of Mercury Oxide, and then divide the molar mass of Oxygen by the molar mass of the compound.

So...

mm of Hg + mm of O= 200.59g + 16g= 217g

16g/217g = .0737... x 100 = 7.37%

6 0

3 years ago

HELP ME PLS I NEED HELP

sesenic [268]

Lol your answer is c

3 0

3 years ago