Acetic acid (ch3cooh) is formed from its elements by the following reaction equation:
2 c (graphite) + 2 h2 (g) + o2 (g) → ch3cooh (g)1. what is the volume of acetic acid ch3cooh gas produced by the reaction of 18.6 grams of h2 gas at 35°c and 1.05 atm?

111 L

Explanation:

Calculation of moles of hydrogen gas:-

Mass of = 18.6 g

Molar mass of = 2.01588 g/mol

According to the given reaction:-

2 moles of hydrogen gas on reaction produces one mole of acetic acid gas.

So,

1 mole of hydrogen gas on reaction produces mole of acetic acid gas.

Also,

9.23 mole of hydrogen gas on reaction produces mole of acetic acid gas.

Moles of acetic acid gas = 4.615 moles

Given that:

Temperature = 35 °C

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

T(K) = T( °C) + 273.15  

So,  

T = (35 + 273.15) K = 308.15 K  

n = 4.615 moles

P = 1.05 atm

V = ?

Using ideal gas equation as:

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:

1.05 atm × V = 4.615 moles ×0.0821 L atm/ K mol  × 308.15 K  

⇒V = 111 L

it takes on an electronical energy

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