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babymother [125]
3 years ago
11

Acetylene is hyrodgenated to form ethane. The feed to the reactor contains 1.60 mol H2/mol C2H2. The reaction proceeds to comple

tion.a. Calculate the stoichiometric reactant ratio (mol H2 reacted/mol C2H2 reacted) and the yield ratio (mol C2H6 formed/mol H2 reacted).
Chemistry
1 answer:
Black_prince [1.1K]3 years ago
4 0

Answer:

Explanation:

C₂H₂     +   2H₂   =     C₂H₆

1 mole     2 mole        1 mole

Feed of reactant is 1.6 mole H₂ / mole C₂H₂

or 1.6 mole of H₂ for 1 mole of C₂H₂

required ratio as per chemical reaction written above

2 mole of  H₂ for 1 mole of C₂H₂

So H₂ is in short supply . Hence it is limiting reagent .

1.6 mole of H₂ will react with half of 1.6 mole or .8 mole of C₂H₂ to form .8 mole of C₂H₆

a )Calculate the stoichiometric reactant ratio =  mole H₂ reacted/mole C₂H₂ reacted

= 1.6 / .8 = 2 .

b )

yield ratio = mole C₂H₆ formed / mole H₂ reacted ) = 0.8 / 1.6 = 1/2 = 0.5 .

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Answer:

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Step-by-step explanation:

a) Balanced equation

Normally, we would need a balanced chemical equation.

However, we can get by with a partial equation, as log as carbon atoms are balanced.

We know we will need an equation with masses and molar masses, so let’s <em>gather all the information</em> in one place.  

M_r:    30.07          236.74

           C₂H₆ + … ⟶ C₂Cl₆ + …  

m/g:    90.0

(i) Calculate the moles of C₂H₆

n = 90.0 g C₂H₆  × (1 mol C₂H₆ /30.07 g C₂H₆)

  = 2.993 mol C₂H₆

(ii) Calculate the moles of C₂Cl₆

The molar ratio is (1 mol C₂Cl₆/1 mol C₂H₆)

n = 2.993 mol C₂H₆ × (1 mol C₂Cl₆/1 mol C₂H₆)

  = 2.993 mol C₂Cl₆

(iii) Calculate the mass of C₂Cl₆

m = 2.993 mol C₂Cl₆ × (236.74 g C₂Cl₆/1 mol C₂Cl₆)

m = 709 g C₂Cl₆

The reaction produces 709 g C₂Cl₆.

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Calculate δg o for each reaction using δg of values:(a) h2(g) + i2(s) → 2hi(g) kj (b) mno2(s) + 2co(g) → mn(s) + 2co2(g) kj (c)
steposvetlana [31]
Part (a) :
H₂(g) + I₂(s) → 2 HI(g)
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Part (b):
MnO₂(s) + 2 CO(g) → Mn(s) + 2 CO₂(g)
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G CO₂ = - 394.39
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Part (c):
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6 0
3 years ago
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