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2 years ago

P4(s) + O2(g) → __ P4O10(s) Now we will balance O. How many O2 molecules are needed to form one P4O10 molecule?

Chemistry

1 answer:

Mnenie [13.5K]2 years ago

4 0

Answer:

Five molecules of oxygen.

Explanation:

Hello,

In this case, considering the given chemical reaction, we must write a five before the oxygen in order to equal the number of oxygen atoms at both the right and left side (ten) so phosphorous remain the same (4):

$P_4(s) + 5 O_2(g)\rightarrow P_4O_{10}(s)$

It means that five molecules of oxygen (O₂) are needed to form one molecule of tetraphosphorous decaoxide (P₄O₁₀).

Best regards.

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2 years ago

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2 years ago

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Answer:

The empirical formula is = $Fe(CO)_2$

Explanation:

Carbon dioxide obtained:

Pressure = 44.9 mm Hg

Also, P (mm Hg) = P (atm) / 760

Pressure = 44.9 / 760 = 0.0591 atm

Temperature = 25 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15

So,

T₁ = (25 + 273.15) K = 298.15 K

V = 1.50 L

Using ideal gas equation as:

PV=nRT

where,

P is the pressure

V is the volume

n is the number of moles

T is the temperature

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.0591 atm × 1.50 L = n × 0.0821 L.atm/K.mol × 298.15 K

⇒n = 0.0036 moles

1 mole of carbon atoms are present in 1 mole of carbon dioxide. So,

Moles of C = 0.0036 moles

Molar mass of C atom = 12.0107 g/mol

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Mass of Fe in the sample = Total mass - Mass of C

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Moles of Fe = 0.0988 / 55.845 = 0.0018 moles

Taking the simplest ratio for Fe and C as:

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The empirical formula is = $Fe(CO)_2$

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2 years ago

__ P4(s) + __ O2(g) → __ P4O10(s) Now we will balance O. How many O2 molecules are needed to form one P4O10 molecule?

P4(s) + O2(g) → __ P4O10(s) Now we will balance O. How many O2 molecules are needed to form one P4O10 molecule?