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nlexa [21]
3 years ago
15

Standard Heat of Formation: The enthalpy change for the formation of 1 mol of a substance in its standard state from its constit

uent elements in their standard states. True/ false?
Chemistry
1 answer:
12345 [234]3 years ago
6 0

The given statement about standard heat of formation is true.

Explanation:

Yes, it is true that standard heat of formation is same as standard enthalpy of formation. As enthalpy is termed for change in the heat energy occurred in the process of completion of any chemical reaction, the standard enthalpy or heat of formation is termed as the heat energy required to form 1 mole of any substance in its standard state from its original, parent or constituent elements in their standard state. Basically, it defines the amount of energy required by the system or compound for its formation from different elements under different synthesis conditions but the nature of the parent samples and temperature and pressure should be kept standard.

So the given statement is true.

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How many moles are there in 32.4 grams of Na
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Divide that my the molar mass which is 23 so 1.4087 g
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Given similar concentrations, the stronger acid corresponds to the lower pH. Comment on the relative strengths of the acids H3PO
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Answer:

H3PO4 is stronger than H2PO4- because

H3PO4 dissociation constant is 6.9×10^-3

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Type the correct answer in the box. Express your answer to three significant figures. Iron(II) chloride and sodium carbonate rea
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Answer:

The reaction can produce 287 grams of iron(II) carbonate

Explanation:

To solve this question we must find the moles of iron(II) chloride that react. Using the chemical equation we can find the moles of iron(II) carbonate and its mass -Molar mass FeCO3: 115.854g/mol-

<em>Moles FeCl2:</em>

1.24L * (2.00mol / L) = 2.48 moles FeCl2

As 1 mol FeCl2 produce 1 mol FeCO3, the moles of FeCO3 = 2.48 moles

<em>Mass FeCO3:</em>

2.48mol * (115.854g / mol) =

<h3>The reaction can produce 287 grams of iron(II) carbonate</h3>
5 0
2 years ago
Rock samples, taken from the Moon, contain many of the same minerals as those found on Earth. Why might this be the case?
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Which ions aren't shown in net ionic reactions, because they are present as both reactants and products of the reaction, so they
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Explanation:

This is correct!

Ions that exist in both the reactant and product side of the equation are referred to as spectator ions. Overall, they do not partake in the reaction. If they are present on both sides of the equation, you can cancel them out.

An example is;

Na+(aq) + Cl​−​​(aq) + Ag​+(aq) + NO​3​−​​(aq) → Na​+​​(aq) + NO​3​−​​(aq) + AgCl(s)

The ions; Na+, NO​3​−​​(aq) would be cancelled out to give;

Cl​−​​(aq) + Ag​+(aq)  → AgCl(s)

7 0
2 years ago
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