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Kobotan [32]
3 years ago
12

Calculate the volume of a sample of iron that has a density of 6.8 g/mL and a mass of 6780 mg.

Chemistry
1 answer:
Veronika [31]3 years ago
8 0

Answer:

m= 6780mg = 6.78g = 6.8g

d= 6.8g/ml

V= m/d

V= 1ml

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If 20 grams of N2 react completely with H2 , how many moles of NH3 are produced? Show Work
Maslowich
This is the balanced eq
N2 + 3H2 -> 2NH3
first you need to find mole of N2 by using
mol = mass ÷ molar mass.
mol N2= 20g ÷ (14.01×2)g/mol
=0.7138mol
then look at the coefficient between H2 and NH3.
it is N2:NH3
1:2
0.7138:0.7138×2
0.7138:1.4276 moles
moles of NH3 = 1.4276 moles
5 0
3 years ago
Why would you add boiling chips/stones to a solution that is to be refluxed? when should you add them?
anygoal [31]
Answer: Boiling chips provide surfaces on which bubbles can form as the liquid boils.

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6 0
3 years ago
Isotopes percent abundance of antimony
Nitella [24]
Antimony has two naturally occurring isotopes. Their abundance is given in the pic attached below
4 0
3 years ago
Write the following number in Standard (Numeric) Form. 5.8x10-5
DerKrebs [107]

Answer:

the answer of this question is 0.000058

4 0
2 years ago
2Fe(s) +3H2SO4(aq) →Fe2(SO4)3(aq) +3H2(g)When 10.3 g of iron are reacted with 14.8 moles of sulfuric acid, what is the percent y
Elden [556K]

Answer:

1040%

Explanation:

To solve this question we must convert the mass of Iron to moles in order to find limiting reactant. With limiting reactant we can find the theoretical moles of hydrogen and theoretical mass:

Percent yield = Actual yield (5.40g) / Theoretical yield * 100

<em>Moles Fe -Molar mass: 55.845g/mol-:</em>

10.3g * (1mol / 55.845g) = 0.184 moles of Fe will react.

For a complete reaction of these moles there are necessaries:

0.184 moles Fe* ( 3 mol H2SO4 / 2 mol Fe) = 0.277 moles H2SO4.

As there are 14.8 moles of the acid, <em>Fe is limiting reasctant.</em>

The moles of H2 produced are:

0.184 moles Fe* ( 3 mol H2 / 2 mol Fe) = 0.277 moles H2

The mass is:

0.277 moles H2 * (2.016g/mol) = 0.558g H2

Percent yield is:

5.40g / 0.558g * 100 = 1040%

It is possible the experiment wasn't performed correctly

7 0
2 years ago
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