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V125BC [204]
3 years ago
12

Consider the ionic compound that is the combination of the Chromium (III) and hydroxide ions. How many chromium atoms would be p

resent in this compound?
Chemistry
1 answer:
kobusy [5.1K]3 years ago
6 0

An ionic compound forms when a metal bonds with a non-metallic element. Metals usually form the cation and non-metal anions. Chromium has an oxidation number of +3 in the compound and charge on hydroxide ion is -1.

Cation here is Cr^{3+}

Anion is the hydroxide ion OH^{-}

So the formula of the compound will be: Cr(OH)_{3}. The compound has one chromium atom and two hydroxide ions.

Therefore, there will be one Chromium atom per each chromium hydroxide compound.

You might be interested in
If you have 150 grams of s8, how many moles of so2 can you make?
ruslelena [56]

Answer : You can make 4.68 moles of SO₂

Explanation:

Step 1 : Write balanced equation.

S₈ can combine with oxygen to form SO₂ gas. The balanced equation for this reaction is written below.

S_{8}  + 8 O_{2} \rightarrow 8 SO_{2}

Step 2 : Find moles of S₈

The formula to calculate mol is

mole = \frac{grams}{MolarMass}

Molar mass of S₈ is 256.5 g/mol

mole = \frac{150grams}{256.5 g/mol}

mole = 0.585 mol

we have 0.585 mol of S₈

Step 3: Use mole ratio to find moles of SO₂

The mole ratio of S₈ and SO₂ can be found using balanced equation which is 1:8

That means 1 mol of S₈ can form 8 moles of SO₂.

Let us use this as a conversion factor to find moles of SO₂

0.585 mol (S_{8}) \times \frac{8 mol (SO_{2})}{1 mol (S_{8})}  = 4.68 mol

Therefore we have 4.68 moles of SO₂

4 0
3 years ago
Read 2 more answers
The partial pressure of in your lungs varies from 25 mm Hg to 40 mm Hg. What mass of can dissolve in 1.0 L of water at 25 °C if
Sonja [21]

The question is incomplete. The complete question is:

The partial pressure of O_2 in your lungs varies from 25 mm Hg to 40 mm Hg. What mass of O_2  can dissolve in 1.0 L of water at 25 degree Celsius if the partial pressure of O_2 is 40 mm Hg.

Answer: 2.12\times 10^{-3}g  

Explanation:

Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.

To calculate the molar solubility, we use the equation given by Henry's law, which is:

C_{O_2}=K_H\times p_{O_2}

where,

K_H = Henry's constant = 1.30\times 10^{-3}mol/Latm

p_{O_2} = partial pressure = 39 mm Hg =  0.051 atm  (760mmHg=1atm)

Putting values in above equation, we get:

C_{O_2}=1.30\times 10^{-3}mol/Latm\times 0.051atm\\\\C_{O_2}= 6.63\times 10^{-5}mol/L

C_{O_2}=6.63\times 10^{-5}mol/L\times 32g/mol=2.12\times 10^{-3}g

Hence, 2.12\times 10^{-3}g  of O_2 can dissolve in 1.0 L of water at 25 °C if the partial pressure of is 39 mm Hg

8 0
2 years ago
Write and balance the equation for the neutralization reaction between phosphoric acid and
Effectus [21]

Answer: H3PO4(aq)+3NaOH(aq)→Na3PO4(aq)+3H2O(l)

Explanation:

7 0
2 years ago
Element X is in Group 2 and element Y is in Group 17. A compound formed between these two elements is most likely to have the fo
Fofino [41]
The answer is:  XY₂ .
_____________________________________
For example:
______________________________________
   MgCl₂  
______________________________________
8 0
3 years ago
Read 2 more answers
How many mL of 0.105 M aqueous NaOH solution are required to neutralize 40.0 mL of 0.210 M aqueous H2SO4 solution?
nevsk [136]

Answer:

160 mL

Explanation:

Given data:

Molarity of NaOH = 0.105 M

Volume of H₂SO₄ = 40.0 mL (40.0/1000 = 0.04 L)

Molarity of H₂SO₄ = 0.210 M

Volume of NaOH required = ?

Solution:

Number of moles of of H₂SO₄:

Molarity = number of moles / volume in L

0.210 M = number of moles / 0.04 L

Number of moles = 0.210 mol/L × 0.04 L

Number of moles = 0.0084 mol

now we will compare the moles of H₂SO₄  with NaOH.

                     H₂SO₄          :           NaOH

                        1                 :             2

                    0.0084          :         2/1×0.0084 = 0.0168 mol

Volume of NaoH:

Molarity = number of moles / volume in L

0.105 M =  0.0168 mol / Volume in L

Volume in L =  0.0168 mol / 0.105 M

Volume in L =  0.16 L

Volume in mL:

0.16 L × 1000 mL/ 1L

160 mL

7 0
3 years ago
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