Which of these elements would form an ion with a charge of -1?

When the temperature goes up, the volume will also go up

Tju [1.3M]

Answer:

Yes it will

An example is ice, when it melts the volume goes up which means it occupies much more space

4 0

3 years ago

Which statement describes the atoms in gas???

marissa [1.9K]

Answer:

Option-D : They move freely in all directions.

Explanation:

The physical properties of gases are well explained by Kinetic Molecular Theory. The key postulates of this theory are;

1) Composition: Gases are made up of small particles called molecules. The size of these molecules is very small as compared to the distance between molecules, therefore the actual volume of molecules is taken negligible as compared to volume occupied by them.

2) Intermolecular Forces: All the gas molecules present in a container behaves independently because they have no force of interactions between them Hence, the attractive forces are taken negligible or too little.

3) Energies: Gas molecules have greater kinetic energy as compared to solids and liquids. Hence, The gas molecules move randomly. They collide with each other and with the walls of the container which causes pressure.

Conclusion:

Therefore, due to large spaces, no interactions, small sizes and high energies the gas particles move freely and there position is not stationary.

8 0

1 year ago

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What is the maximum mass of ammonia (NH3) that can be produced from the synthesis reaction of 781 g of nitrogen and 656 g hydrog

Daniel [21]

N2(g)+3H2 >>>>>2NH3(g)

the mole ratio between N2, H2 and NH3. It is 1 : 3 : 2

mole N2 present
moles H2 present = 25.0 g H2 x 1 mole H2/2 g = 12.5 moles H2 present
Based on mole ratio, N2 is limiting in this situation because there is more than enough H2 but not enough N2.

moles NH3 that can be produced = 1 mole N2 x 2 moles NH3/mole N2 = 2 moles NH3 can be produced
grams of NH3 that can be produced = 2 moles NH3 x 17 g/mole = 34 grams of NH3 can be produced

5 0

2 years ago

You want to determine the value of x in hydrated iron II sulfate, FeSO4 xH2O. In the laboratory you weigh out 1.983 g of the hyd

jek_recluse [69]

Answer:

The value of x is 7.

Explanation:

When a hydrated salt is heated, the water evaporates because it has a lower boiling point (373 K) and what remains is the anhydrous salt (without water) The mass of the hydrated salt is equal to the sum of the anhydrous salt and the water. Since we have 2 of these 3 data, we can look for the mass of water.

mass of FeSO₄.xH₂O = mass of FeSO₄ + mass of H₂O

mass of H₂O = mass of FeSO₄.xH₂O - mass of FeSO₄

mass of H₂O = 1.983g - 1.084g = 0.899g

This means that 0.899g of water accompany 1.084 g of the salt. We want to know how many grams of water accompany 1 mol of the salt (in the molecular formula we have 1 mol of FeSO₄). Since the molar mass of is 152g/mol, we can establish:

$1mol(FeSO_{4} ).\frac{152gFeSO_{4}}{1mol(FeSO_{4} )} .\frac{0.899gH_{2}O }{1.084gFeSO_{4}} =126gH_{2}O$

As a result 1 mol of FeSO₄ is accompanied by 126 g of water. If we pass that mass into moles:

$126gH_{2}O.\frac{1molH_{2}O}{18gH_{2}O} =7molH_{2}O$

Finally, the number of moles of water in the molecular formula is x = 7.

3 0

3 years ago

495 cm3 of oxygen gas and 877 cm3 of nitrogen gas, both at 25.0 C and 114.7 kpa, are injected into an evacuated 536 cm3 flask. F

I am Lyosha [343]

Answer:

Total pressure of the flask is 2.8999 atm.

Explanation:

Given data:

Volume of oxygen (O2) gas= 495 cm3

= 0.495 L (1 cm³ = 1 mL = 0.001 L)

Volume of nitrogen (N2) gas = 877 cm3

= 0.877 L (1 cm³ = 1 mL = 0.001 L)

volume of falsk = 536 cm3

= 0.536 L (1 cm³ = 1 mL = 0.001 L)

Temperature = 25 °C

T = (25°C + 273.15) K

= 298.15 K

Pressure = 114.7 kPa

= 114.700 Pa

Pressure (torr) = 114,700 / 101325

= 1.132 atm

Formula:

PV=nRT (ideal gas equation)

P = pressure

V = volume

R (gas constnt)= 0.0821 L.atm/K.mol

T = temperature

n = number of moles for both gases

Solution:

Firstly we will find the number of moles for oxygen and nitrogen gas.

For Oxygen:

n = PV / RT

n = 1.132 atm × 0.495 L / 0.0821 L.atm/K.mol × 298.15 K

= 0.560 / 24.47

= 0.0229 moles

For Nitrogen:

n = PV / RT

n = 1.132 atm × 0.877 / 0.0821 L.atm/K.mol × 298.15 K

n = 0.992 / 24.47

= 0.0406

Total moles = moles for oxygen gas + moles for nitrogen gas

= 0.0229 moles + 0.0406 moles

n = 0.0635 moles

Now put the values in formula

PV=nRT

P = nRT / V

P = 0.0635 × 0.0821 L.atm/K.mol × 298.15 K / 0.536 L

P = 1.554 / 0.536

P = 2.8999 atm

Total pressure in the flask is 2.8999 atm, while assuming the temperature constant.

7 0

3 years ago

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