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dlinn [17]
3 years ago
9

Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts wit

h solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.0 kg of SiO2 is allowed to react with 79.0 kg of carbon to produce 66.2 kg of silicon.
A. Which is the limiting reactant?
B. What is the theoretical yield?
C. What is the percent yield?
Chemistry
1 answer:
riadik2000 [5.3K]3 years ago
5 0

Answer:

A) SiO2 is the limiting reactant

B) Theoretical yield= 72333.3g

C) % yield =91.5%

Explanation:

SiO2(s) + 2C(s) --------------> Si(s) + 2CO(g)

n(SiO2)= 155000/60 = 2583.33 mols

n(C)= 79000/12= 3291.66 mols

a)SiO2 is the limiting reactant

According to the balanced reaction equation,

60g of SiO2 produced 28g of SiO2

155000g of SiO2 will produce 155000×28/60= 72333.3g

Therefore theoretical yield of Si= 72333.3g

% yield= 66200/72333.3×100/1 =91.5%

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kogti [31]

Answer:

c is right

Explanation:

8 0
2 years ago
What is the percent yield of a reaction in which 200. g of phosphorus trichloride reacts with excess water to form 91.0 g of hcl
Snowcat [4.5K]
Answer is: <span>yield of a reaction is 56,4%.
</span>Chemical reaction: PCl₃ + 3H₂O → 3HCl + H₃PO₃.
m(PCl₃) = 200 g.
m(HCl) = 91,0 g.
n(PCl₃) = m(PCl₃) ÷ M(PCl₃).
n(PCl₃) = 200 g ÷ 137,33 g/mol.
n(PCl₃) = 1,46 mol.
n(HCl) = m(HCl) ÷ M(HCl).
n(HCl) = 91 g ÷ 36,45 g/mol.
n(HCl) = 2,47 mol.
From reaction: n(PCl₃) : n(HCl) = 1 : 3.
n(HCl) = 1,46 mol · 3 = 4,38 mol.
Yield of reaction: 2,47 mol ÷ 4,38 mol · 100% = 56,4%.
4 0
3 years ago
Read 2 more answers
Which of the following molecules has one lone pair of electrons?
BigorU [14]
You can automatically rule out CH₄ since it has no lone pairs at all around the central atom. Water has 2. Ammonia is the only Lewis structure that contains one lone pair.
7 0
2 years ago
Read 2 more answers
Density, Mass, or Volume is a physical property of matter?
ohaa [14]
Density is a physical property of matter
4 0
3 years ago
A chemist adds of a calcium sulfate solution to a reaction flask. Calculate the mass in grams of calcium sulfate the chemist has
Elanso [62]

The given question is incomplete. The complete question is:

A chemist adds 0.85 L of a 0.0050M calcium sulfate to a reaction flask. Calculate the mass in grams of calcium sulfate the chemist has added to the flask. Round your answer to significant digits.

Answer: The mass in grams of calcium sulfate the chemist has added to the flask is 0.58 g

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

Molarity=\frac{n}{V_s}

where,

n = moles of solute

V_s = volume of solution in L

moles of CaSO_4 = \frac{\text {given mass}}{\text {Molar mass}}=\frac{xg}{136g/mol}

Now put all the given values in the formula of molarity, we get

0.0050=\frac{x}{136\times 0.85}

x=0.58 g

Therefore, the mass in grams of calcium sulfate the chemist has added to the flask is 0.58 g

7 0
3 years ago
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