If Ca+2 would react with F-1, what do you predict to be the formula

Chemistry

1 answer:

ollegr [7]3 years ago

3 0

It would be CaF2 because you will need to balance then so since F is -1 it'll need another one to balance with Ca +2

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Aluminum oxide (Al2O3) occurs in nature as a mineral called corundum, which is noted for its hardness and resis- tance to attack

Neko [114]

Answer:

7.03×10²³ atoms of Al

Explanation:

Corundum density = 3.97g/cm³

Corundum = Al₂O₃. Then, you have 2 moles of Al and 3 moles of O in 1 mol of the compound.

Let's determine the mass of corundum, by density

Corundum density = Corundum mass / Corundum volume

3.97 g/cm³ = Corundum mass / 15cm³

3.97 g/cm³ . 15cm³ = Corundum mass →59.55 g

Now, let's find out how many moles are in that mass of corundum

1 mol of Al₂O₃ weighs 101.96 g/mol

Then, 101.96 grams of oxide have 2 moles of Al

59.55 g of oxide, will have (59.55 .2)/101.96 = 1.17 moles

Now, we can know the quantity of atoms, by this rule of three

1 mol has NA atoms (6.02×10²³)

1.17 moles will have (1.17 . NA) = 7.03×10²³ atoms of Al

5 0

3 years ago

How does the bond energy of HCl(g) differ from the standard enthalpy of formation of HCl(g)?

sergeinik [125]

Answer:

it's the same if rounded off to the nearest decimal or slightly different if not.

Explanation:

The enthalpy of formation is -431.6 kJ, while the bond energy of H-Cl is -432 kJ.

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3 years ago

An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d = 1.114 g/ml; = 62.07 g/mol) and water (d

tankabanditka [31]

a) Volume percent

Formula: % v/v = [volume solute / volume solution] * 100

Just to make it easy take a base of 50 volume parts of ethylen glycol and 50 volume parts of water to make 100 volumes of mixture (this assumpion will be valid for all the questions):

% v/v =[ 50 ml ethyleneglycol] / [100 ml mixture] * 100 = 50%

Answer: 50% v/v

b) Mass percent

% m/m = [mass ethylene glycol / mass solution] * 100

mass ethylene glycol = 50 ml * 1.114 g/ ml = 55.7 g

mass of mixture = 100 ml * 1.07 g/ml = 107 g

% m/m = [55.7 / 107 g] * 100 = 52.06 %

Answer: 52.06%

c) Molarity

M = number of moles of solute / liters of solution

number of moles of solute = mass in grams / molar mass

number of moles of ehtylene glycol = 55.7 g / 62.07 g/mol = 0.8974 mol

liters of solution = 0.1 liter

M = 0.8974 mol / 0.1 liter = 8.974 M

Answer: 8.974 M

d) Molality

m = number of moles of solute / kg of solvent

number of moles of ethylen glycol = 0.8974 mol

mass of water = 50 ml * 1 g/ml = 50 g = 0.05 kg

m = 0.8974 mol / 0.05 kg = 17.95 m

Answer: 17.95 m

e) mole fraction

mole fraction = [number of moles of solute] / [number of moles of mixture] * 100

number of moles of ethylen glycol = 0.8974 mol

number of moles of water = 50 g / 18.01 g /mol = 2.776 mol

mole fraction = 0.8974 mol / [0.8974 mol + 2.776 mol] = 0.244

Answer: 0.244

7 0

3 years ago

For the decomposition of ammonia on a platinum surface at 856 °C

Crazy boy [7]

$\\ \tt\leadsto \dfrac{d[NH_3]}{dt}=1.50\times 10^{-6}$