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il63 [147K]
3 years ago
10

4.00 g of O2 gas are in a sealed, 2.00 L gas canister at 22.0 °C what is the pressure inside this container (in atm)?

Chemistry
1 answer:
Volgvan3 years ago
6 0

Answer:

1.51448 atms

Explanation:

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use the periodic table to select the element from the drop-down menu that has the correct relative electronegativity.
Bumek [7]
You need to list the elements but remember that fluorine has the highest electronegativity out of the entire periodic table
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3 years ago
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What is the [OH-],[H3O] and PH for the following
malfutka [58]

The values for hydroxide ions, hydronium ions and pH are found in the attached picture.

Explanation:

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4 0
3 years ago
Calculate the number of kilojoules to warm 125 g of iron from 23.5 °C to 78.0 °C.
insens350 [35]
Given:
Iron, 125 grams T
1 = 23.5 degrees Celsius, T2 = 78 degrees Celsius.  

Required:
Heat produced in kilojoules  

Solution:
The molar mass of iron is 55.8 grams per mole. SO we need to change the given mass of iron into moles.  
 
Number of moles of iron = 125 g/(55.8 g/mol) = 2.24 moles  
<span>
Q (heat) = nRT = nR(T2 = T1)</span>
Q (heat) = 2.24 moles (8.314 Joules per mol degrees Celsius) (78.0 degrees Celsius – 23.5 degrees Celsius)
<u>Q (heat) = 1014.97 Joules or 1.015 kilojoules</u> <span>This is the amount of heat produced in warming 125 g f iron.</span>
7 0
3 years ago
4 g of ag2so4 will dissolve in 1l of water. calculate the solubility product (ksp) for silver (i) sulfate.
Bas_tet [7]
Reaction of dissociation: Ag₂SO₄ → 2Ag⁺ + SO₄²⁻.
m(Ag₂SO₄) = 4 g.
V(Ag₂SO₄) = 1 l.
n(Ag₂SO₄) = m(Ag₂SO₄) ÷ M(Ag₂SO₄).
n(Ag₂SO₄) = 4 g ÷ 311,8 g/mol.
n(Ag₂SO₄) = 0,0128 mol.
n(Ag⁺) = 2 · 0,0128 mol = 0,0256 mol.
n(Ag₂SO₄) = n(SO₄²⁻) = 0,0128 mol.
c(Ag⁺) = n ÷ V = 0,0256 mol ÷ 1 l = 0,0256 mol/l.
Ksp = c(Ag⁺)² · c(SO₄²⁻).
Ksp = (0,0256 mol/l)² · 0,0128 mol/l.
Ksp = 8,3·10⁻⁶.

7 0
3 years ago
What do two or more atoms form when they share electrons in a chemical bond
dlinn [17]
A covalent bond is your answer
6 0
3 years ago
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