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3 years ago

What is the mass of 2.56 × 10–4 moles of Fe2O3? : 6.23 × 105 159.6 g 1.60 × 0–6 g 4.09 × 10–2 g

Chemistry

1 answer:

Monica [59]3 years ago

7 0

Answer:

4.09 × 10⁻² g

Solution:

As we know that,

1 mol of Fe₂O₃ is equal to = 159.69 g

So,

2.56 × 10⁻⁴ mol will be equal to = X g

Solving for X,

X = (159.69 g × 2.56 × 10⁻⁴ mol) ÷ 1 mol

X = 0.04088 g

Or,

X = 0.049 g

Or,

X = 4.09 × 10⁻² g

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4 years ago

What is the volume of an oxygen tank if it contains 12 moles of oxygen at 273 K under 75 kPa?

Zina [86]

Given:
n = 12 moles of oxygen
T = 273 K, temperature
p = 75 kPa, pressure

Use the ideal gas law, given by
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4 years ago

What is the concentration of 10.00 mL of HBr if it takes 16.73 mL of a 0.253 M LiOH solution to neutralize it?

Leni [432]

First. let's write the reaction formula: HBr +LiOH ----> LiBr + H₂O

let's get the moles of LiOH first

moles= Molarity x Liters

moles= 0.253 M x 0.01673 Liter= 0.00423 moles LiOH

using the balanced equation, you can see that 1 mol LiOH is equal to 1 mol HBr. so:

0.00423 mol LiOH = 0.00423 mol HBr

now let's find the concentration

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4 years ago