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Chapter 3: Q45E (page 83)

Question:The percent by mass of nitrogen for a compound is found to be 46.7%. Which of the followingcould be this species?

Short Answer

Expert verified

Answer

NO could be this species.

Step by step solution

Finding the number of moles of N and O

To calculate the percentage for O can be,

$100 % - 46.7 % = 53.3 %$

The masses of N and O in 100 gram sample can be calculated as,

$46.7 % . 100 g = 46.7 g N 53.3 % . 100 g = 53.3 g O$

To find the moles number can be calculated as,

$O : 16 g / m o l, N : 14.01 g / m o l$

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Most popular questions from this chapter

Consider the following reaction:

$4 {NH}_{3} (g) + 5 O_{2} (g) \to 4 NO (g) + 6 H_{2} O (g)$

If a container were to have 10 molecules of

O_{2}

and 10 molecules of

{NH}_{3}

initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?

Iron oxide ores, commonly a mixture of $FeO$ and ${Fe}_{2} O_{3}$ are given the general formula ${Fe}_{3} O_{4}$ .
They yield elemental iron when heated to a very high temperature with either carbon monoxideor elemental hydrogen. Balance the following equations for these processes:

${Fe}_{3} O_{4} (s) + H_{2} (g) \to Fe (s) + H_{2} O (g)$

${Fe}_{3} O_{4} (s) + CO (g) \to Fe (s) + {CO}_{2} (g)$

Which of the following statements about chemical equations is (are) true?

When balancing a chemical equation, you can never change the coefficient in front of anychemical formula.
The coefficients in a balanced chemical equation refer to the number of grams of reactantsand products.
In a chemical equation, the reactants are on the right and the products are on the left.
When balancing a chemical equation, you can never change the subscripts of any
formula.
In chemical reactions, matter is neither created nor destroyed so a chemical equation must have the same number of atoms on both sides of the equation.

Question:The atomic mass of boron (B) is given in the periodic table as 10.81, yet no single atom of boronhas a mass of 10.81 u. Explain.

Phosphorus can be prepared from calcium phosphate by the following reaction:

${2Ca}_{3} {({PO}_{4})}_{2} (s) {+6SiO}_{2} (s) +10C (s) {→6CaSiO}_{3} (s) {+P}_{4} (s) + 10CO (g)$

Phosphorite is a mineral that contains ${Ca}_{3} {({PO}_{4})}_{2}$ plus other non-phosphorus-containing compounds. What is the maximum amount of $P_{4}$ ,that can be produced $1 kg$ from of phosphorite ,if the phosphorite sample is $75 % {Ca}_{3} {({PO}_{4})}_{2}$ by mass? Assume an excess of the other reactants.

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Question:The percent by mass of nitrogen for a compound is found to be 46.7%. Which of the followingcould be this species?

Short Answer

Step by step solution

Finding the number of moles of N and O

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Most popular questions from this chapter

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