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3 years ago

FIRST GETS BRAINLIEST

Chemistry

1 answer:

lisov135 [29]3 years ago

8 0

Answer:

0.07172 L = 7.172 mL.

Explanation:

We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm (P = 1.0 atm, Standard P).

V is the volume of the gas in L (V = ??? L).

n is the no. of moles of the gas in mol (n = 3.2 x 10⁻³ mol).

R is the general gas constant (R = 0.0821 L.atm/mol.K),

T is the temperature of the gas in K (T = 273 K, Standard T).

∴ V = nRT/P = (3.2 x 10⁻³ mol)(0.0821 L.atm/mol.K)(273 K)/(1.0 atm) = 0.07172 L = 7.172 mL.

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The empirical formula of the oxide is Co₂O₃.

Step 1. Calculate the mass of oxygen

Your reaction is

Cobalt + oxygen ⟶ cobalt oxide

29.05 g + x g ⟶ 40.88 g

According to the Law of Conservation of Mass, the total mass of the reactants must equal the total mass of the products. Thus,

29.05 g + x g ⟶ 40.88 g

x = 40.88 – 29.05 = 11.83

Step 2. Calculate the moles of each element

The empirical formula is the simplest whole-number ratio of atoms in a compound.

The ratio of atoms is the same as the ratio of moles.

So, our job is to calculate the molar ratio of Co to O.

Moles of Co = 29.05 g Co × (1 mol Co /(58.93 g Co) = 0.492 96 mol Co

Moles of O = 11.83 g O × (1 mol O/16.00 g O) = 0.739 38 mol O

Step 3. Calculate the molar ratio of the elements

Divide each number by the smaller number of moles

Co:O = 0.429 26:0.739 38 = 1:1.4999

Step 4. Multiply each number by a factor that makes the ratio close to whole numbers

Multiply by 2. Then

Co:O = 2:2.998 ≈ 2:3

Step 5: Write the empirical formula

EF = Co₂O₃

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Answer:

ΔH for formation of 197g Fe⁰ = 1.503 x 10³ Kj => Answer choice 'B'

Explanation:

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