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Citrus2011 [14]
3 years ago
12

How many grams of nitric acid will react completely with a block of iron metal that is 4.5 cm by 3.0 cm by 3.5 cm, if the densit

y of iron is 7.87 g/mL? Show all steps of your calculation as well as the final answer. Fe + HNO3 → Fe(NO3)3 + H2
Chemistry
2 answers:
oksano4ka [1.4K]3 years ago
8 0

Answer:

1258 g HNO3

Explanation:

First, we need to calculate the grams of Fe we have using the density and the volume given. For this, use the definition of density which is:

Density = mass / volume

So

Mass = Density x volume

For the statement, the volume of Fe will be:

Volume = (4.5 cm)(3.0 cm)(3.5 cm) = 47.2 cm^3

And as 1 cm^3 is equal to 1 mL, then:

Volume = 47.2 mL

So the mass of Fe we have is:

Mass = (7.87 g/mL)(47.2 mL) = 371.9 g Fe

To find the amount of nitic acid that reacts we need to work with moles, then:

Moles of Fe = 371.9gFe (\frac{1 mole Fe}{55.85 gFe})=6.658 moles Fe

And as the balanced reaction is  2Fe + 6HNO3 → 2Fe(NO3)3 + 3H2, then the moles of nitric acid that reacts with the given amount of iron is:

Moles of HNO3 = 6.658moleFe (\frac{6 moles HNO3}{2 moles Fe} )=19.97 moles HNO3

But they are asking for the grams that react, so we need the molecular mass of HNO3 to do the conversion

Molecular mass of HNO3 = 1.008 g H + 14.01 g N + 3(16.00 g O) = 63.02 g HNO3

Finally, the mass of HNO3 that reacts with the amount of iron given is:

mass HNO3 = 19.97molesHNO3 (\frac{63.02 g HNO3}{1 mole HNO3} ) = 1258 g HNO3

denpristay [2]3 years ago
7 0

Balance the equation first: 

2 Fe+6 HNO3→2 Fe(NO3)3+3H2

Then calculate mass of Iron :

4.5×3.0×3.5 cm3(1 mL1 cm3)(7.87 g Fe1 ml)=371.86 g Fe

Now use Stoichiometry:

371.86 g Fe×(1 mol Fe55.85 g Fe)×(6 mol HNO32 mol Fe)=19.97 mol HNO3

Convert moles of nitric acid to grams

19.97 mol HNO3×(63.01 g HNO31 mol HNO3)=1258.3 g HNO3



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How many grams of HNO3 are produced when 60.0 g of NO2 completely reacts?
olganol [36]
<h3>Answer:</h3>

54.756 g

<h3>Explanation:</h3>

Assuming the equation for the reaction in question;

3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)

We are given;

  • Mass of NO₂ as 60.0 g

We are required to calculate the mass of HNO₃ produced

  • We can calculate the mass of HNO₃ produced using the following simple steps;
<h3>Step 1: Calculate the moles of NO₂</h3>

Moles = Mass ÷ Molar mass

Molar mass of NO₂ = 46.01 g/mol

Therefore;

Moles of NO₂ = 60.0 g ÷ 46.01 g/mol

                       = 1.304 moles

<h3>Step 2: Calculate the moles of HNO₃ produced </h3>

From the equation, 3 moles of NO₂ reacted to produce 2 mole of HNO₃

Therefore, the mole ratio of NO₂ to HNO₃ is 3 : 2

Thus;

Moles of HNO₃ = Moles of NO₂ × 2/3

                          = 1.304 moles × 2/3

                          = 0.869 Moles

<h3>Step 3: Calculate the mass of HNO₃</h3>

Mass = Moles × Molar mass

Molar mass of HNO₃ = 63.01 g/mol

Therefore;

Mass = 0.869 moles × 63.01 g/mol

         = 54.756 g

Thus, the mass of HNO₃ produced is 54.756 g

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3 years ago
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Answer:

The correct answer is 25 mL graduated cylinder (it should be used in all the cases)

Explanation:

In order to measure 25.00 ml sample of a solution it should be used a 25 mL graduated cylinder, as it is previously and properly calibrated. The other laboratory glassware, beaker and erlenmeyer, have graduations which are approximate, so they are used when exact volumes are not needed.

ii) graduated cylinder has the least uncertainly. It is more accurate than a beaker or erlenmeyer (to within 1%)

iii) A 25 mL graduated cylinder should be used because it is the most accurate lab glassware (between those were mentioned: beaker, erlenmeyer).

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Answer:

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The vertical columns on the periodic table are called groups or families because of their similar chemical behavior. All the members of a family of elements have the same number of valence electrons and similar chemical properties. The horizontal rows on the periodic table are called periods.

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