Elements in the same group have the same _ and __

Chemistry

1 answer:

OlgaM077 [116]3 years ago

6 0

Answer:

Elements in the same group have the same number or valence electrons and similar chemical properties.

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The density of a sample of F2(g) is 1.559 g/L. If the gas is held at 755 torr, calculate the temperature.

4vir4ik [10]

Answer:

The temperature is 590,10 K

Explanation:

As stated, we understand that there is one mole of F2, which is equivalent to 37.9968x2 grams = 75.936 grams. The unit of Torr is converted to atm, 1 Torr = 0.0013 atm, and with the data of grams it is converted into volume through density:

density = m / v ---> v = m / density = 75,936 g / 1,559 g / l = 48, 708 l

Exactly the formula PV = nRT

n = number of moles (according to what is interpreted in the sentence is 1 mole)

P = pressure 755 Torr (converted to atm 755Torr / 0.0013 atm / Torr = 0.99344 atm)

R = value constant 0.082 l x atm / K x mol

T = is our mystery (in degrees Kelvin)

0.99344 x 48, 708 l = 1 mol x 0.082 l x atm / K x mol x X

X = 0.99344 x 48, 708 l / 1 mol x 0.082 l x atm / K x mol

X = 590, 10 K

The temperature is 590.10 K

7 0

3 years ago

How many total moles of ions are released when each of the following dissolves in water?

Gnom [1K]

Thus 3 moles of ions are released when samples dissolves definitely in water.

Water (H2O) is made from 2 atoms of hydrogen and 1 atom of oxygen. A mole of water molecules would be 2 moles of hydrogen atoms plus 1 mole of oxygen atoms.

One mole of a substance is equal to 6.022 × 10²³ units of that substance (such as atoms, molecules, or ions). The variety 6.022 × 10²³ is acknowledged as Avogadro's number or Avogadro's constant.

<h3>How plenty is a mole of water?</h3>

18.0146 grams

The atomic mass of hydrogen is 1.0078 and the atomic mass of oxygen is 15.999, so the mass of a mole of water is two x 1.0078 + 15.999. Therefore, a mole of water, or 6.022 x 1023 molecules, weighs 18.0146 grams.

Learn more about moles of ion here:

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5 0

2 years ago

How does the presence of hcl affect the charges on the complexes?

FrozenT [24]

Hydrochloric Acid (HCl) is a strong acid when it is present in the concentrated form but when it is dissolved in water ( $H_2O$ ) the atoms of this compound dissociates into its respective ions as shown below:

$HCl(aq.) + H_2O(aq.) \rightarrow H_3O^+(aq.) + Cl^-(aq.)$

When we add HCl to any complex in its concentrated form the complex does not react at all but when its diluted to 6M and is kept for many hours, the complex reacts slowly. For eg:

$[Co(NH_3)_6]^3^+(aq.) + HCl(aq.) \rightarrow [Co(NH_3)_5Cl]^2^+(aq.) + NH_4^+ (aq.)$

As seen from the above reaction it can be seen the positive charge on the complex is reduced by 1 unit because one $Cl^-$ ion gets attached to the centre metal atom, therefore we can conclude that the charge on complex gets reduced by 1 unit when HCl reacts with the complex.