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2 years ago

How many equivalents are in 0.60 mole of Mg2+

1 answer:

5 0

Equivalents express the combining power of an element for example what mass of an element can combine with or displace one gram of hydrogen or eight grams of oxygen.

Since Mg is divalent, one gram of Mg2+ can combine with 2 grams of hydrogen

Therefore, 0.6 mole of Mg2+ can combine with 0.6 x 2 = 1.2 moles of hydrogen

Hence there are 1.2 equivalents in 0.60 mole of Mg2+

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You start with a container that is 8L big and the temperature in the room is 326K.

Ket [755]

Answer:

The new volume is 8.64 L.

Explanation:

Charles's Law consists of the relationship that exists between the volume and the temperature of a certain quantity of ideal gas, which is maintained at a constant pressure. For a given sum of gas at constant pressure, as the temperature increases, the volume of the gas increases and as the temperature decreases, the volume of the gas decreases.

In summary, Charles's law is a law that says that when the amount of gas and pressure are kept constant, the quotient that exists between the volume and the temperature will always have the same value:

$\frac{V}{T} =k$

Being an initial state 1 that modifies its conditions until a final state 2, it is fulfilled:

$\frac{V1}{T1} =\frac{V2}{T2}$

In this case:

V1= 8 L
T1= 326 K
V2= ?
T2= 352 K

Replacing:

$\frac{8L}{326 K} =\frac{V2}{352 K}$

Solving:

$V2=352 K*\frac{8L}{326 K}$

V2= 8.64 L

<u><em>The new volume is 8.64 L.</em></u>

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1 year ago

Which career area in chemistry applies new discoveries to practical applications useful for consumers?

levacccp [35]

I think it would be D

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2 years ago

If 1.00 mol of argon is placed in a 0.500-L container at 20.0 ∘C , what is the difference between the ideal pressure (as predict

antiseptic1488 [7]

Hey There!

ideal gas law :

PV = nRT

P = nRT/V

P = (1*0.082)(18+273)/(0.5) = 47.724 atm

For VDW :

(P + a(n/V)²)(V - nB) = nRT

P = nRT/(V - nB) - a(n/V)²

P = 1*0.082*(18+273) / (0.5-1*0.03219) - 1.345*( 1/0.5 )² = 45.62

P = 45.62 atm

Pdif = P2-P1 = 47.724 - 45.62 = 2.104 atm

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As a hydrated compound is heated, it decreases in

Sergio [31]

A hydrated substance will decrease in mass when heated since the water is being boiled away.

I hope this helps. Let me know if anything is unclear.

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How was Earth’s atmosphere changed during the Great Oxygenation Event?

SpyIntel [72]

Consequences of oxygenation. Eventually, oxygen started to accumulate in the atmosphere, with two major consequences. Oxygen likely oxidized atmospheric methane (a strong greenhouse gas) to carbon dioxide (a weaker one) and water.

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1 year ago

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