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4 years ago

What mass of iron (Fe) can be obtained from 3.80 g iron (III) oxide (Fe2O3) reacting with excess carbon monoxide (CO)?

Chemistry

1 answer:

Vadim26 [7]4 years ago

5 0

Answer:

2.66 g of Fe, can be obtained from the reaction

Explanation:

Let's think the reaction:

2Fe₂O₃ + 6CO → 4Fe + 6CO₂

Ratio is 2:4, so If i have x moles of iron (III) oxide, I will produce the double of moles of Fe.

Mass / Molar mass = Mol

3.80 g / 159.7 g/m = 0.0237 moles

0.0237 moles . 2 = 0.0475 moles

Molar mass Fe = 55.85 g/m

Mol . Molar mass = Mass → 0.0475 m . 55.85 g/m = 2.66 grams

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Tris is a weak base. The basic form of tris can be written tris0 and the protonated (conjugate acid) form can be written tris. T

Arada [10]

Answer:

a) [Tris0] : [Tris] = 1 : 100

b) Range = 7.1 to 9.1

Explanation:

a) Calculation of ratio of the basic and the acidic forms of tris

pH of a buffer is calculate using Henderson-Hasselbalch equation

$pH = pKa+log\frac{Salt}{Acid}$

Conjugate acid of Tris dissociated as

$Tris \leftrightharpoons Tris0 + H^+$

For tris,

Salt or Basic form = tris0

Acid or Acidic form = Tris

pKa = 8.1

pH = 6.1

$pH = pKa+log\frac{Tris0}{Tris}$

$6.1 = 8.1+log\frac{Tris0}{Tris}$

$log\frac{Tris0}{Tris} = -2$

$\frac{Tris0}{Tris} = antilog (-2)$

$\frac{Tris0}{Tris} = 10^{-2}$

[Tris0] : [Tris] = 1 : 100

b) Range of Tris

Range of any buffer is:

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3 years ago

A sample of potassium phosphate octahydrate (K3PO4•8H2O) is heated until 7.93 grams of water are released. How many grams did th

Gekata [30.6K]

The original sample of potassium phosphate octahydrate had a mass of 19.6 grams. When it was heated, it released 7.93 grams of water.

Further Explanation:

For every mole of the compound potassium phosphate octahydrate, there are 8 moles of water of hydration which can be removed from the crystal by heating without altering the chemical composition of the substance.

To determine how much original sample was used, the amount of water released upon heating may be used as well as the mole ratio of the water of hydration with the compound itself following the steps below:

Convert mass of water released to moles.
Use the mole ratio of water of hydration to the compound (8 mol water for every mol of potassium phosphate octahydrate) to get the moles of original sample.
Convert the moles of original sample to grams.

STEP 1: Convert 7.93 g water to moles.

$moles \ of\ H_{2}O \ = 7.93 \ g \ H_{2}O \ (\frac{1 \ mol \ H_{2}O}{18.00 \ g \ H_{2}O})\\\boxed {moles \ of \ H_{2}O \ = 0.4406 \ mol}$

STEP 2: Calculate the moles of original sample using the mole ratio: 1 mol K3PO4 8H2O : 8 mol H2O.

$moles \ of \ K_{3}PO_{4}\ 8H_{2}O \ = 0.4406 \ mol \ H_{2}O \ (\frac{1 \ mol \ K_{3}PO_{4}\ 8H_{2}O \ }{8 \ mol \ H_{2}O})\\\\\boxed {moles \ of \ K_{3}PO_{4}\ 8H_{2}O \ = 0.0551 \ mol}$

STEP 3: Convert the moles of original sample to mass.

$mass \ of \ K_{3}PO_{4}\ 8H_{2}O = 0.0551 \ mol \ K_{3}PO_{4}\ 8H_{2}O \ (\frac{356.3885 \ g}{1 \ mol\ K_{3}PO_{4}\ 8H_{2}O})\\ mass \ of \ K_{3}PO_{4}\ 8H_{2}O \ = 19.637 \ g$

Following the significant figures of the given, the final answer should be:

$\boxed {mass \ of \ K_{3}PO_{4}\ 8H_{2}O = 19.6 \ g}$

Learn More:

Learn more about water of hydration brainly.com/question/6053815
Learn more about mole conversion brainly.com/question/12979299
Learn more about percent hydrate brainly.com/question/12398621

Keywords: water of hydration, hydrate

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