1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
9966 [12]
2 years ago
13

A sample of a compound is analyzed and found to contain 0.420 g nitrogen, 0.480g oxygen, 0.540 g carbon and 0.135 g hydrogen. Wh

at is the empirical formula of the compound? a. C2H5NO b. CH3NO c. C3H9N2O2 d. C4HN3O4 e. C4H13N3O3
Chemistry
1 answer:
Crazy boy [7]2 years ago
7 0

Answer:

c. C3H9N2O2

Explanation:

The empirical formula of a compound is defined as the simplest whole number ratio of atoms present in a molecule. To solve this question we need to convert the mass of each atom to moles. With the moles we can find the ratio as follows:

<em>Moles N -Molar mass: 14.01g/mol-</em>

0.420g N * (1mol/14.01g) = 0.0300 moles N

<em>Moles O -Molar mass: 16g/mol-</em>

0.480g O * (1mol/16g) = 0.0300 moles O

<em>Moles C -Molar mass: 12.01g/mol-</em>

0.540g C * (1mol/12.01g) = 0.0450 moles C

<em>Moles H -Molar mass: 1.0g/mol-</em>

0.135g H * (1mol/1g) = 0.135moles H

Dividing in the moles of N (Lower number of moles) the ratio of atoms is:

N = 0.0300 moles N / 0.0300 moles N = 1

O = 0.0300 moles O / 0.0300 moles N = 1

C = 0.0450 moles C / 0.0300 moles N = 1.5

H = 0.135 moles H / 0.0300 moles N = 4.5

As the empirical formula requires whole numbers, multiplying each ratio twice:

N = 2, O = 2, C = 3 and H = 9

And the empirical formula is:

<h3>c. C3H9N2O2</h3>

You might be interested in
What is the approximate ratio of [NO2-] to [HNO2] in order to buffer a solution at pH=4.0?
Strike441 [17]
For the equilibrium that exists in an aqueous solution<span> of nitrous acid (</span>HNO2, a weak acid) ... [H+][NO2. –]. [HNO2<span>]. PAGE: 14.1. 2. Which of the following is a conjugate ... Using the following Ka values, indicate the correct </span>order<span> of base strength. </span>HNO2<span>. Ka = </span>4.0<span> × 10–4 .... Calculate the [H+] in a </span>solution<span>that has a </span>pH<span> of 11.70.
i hope thid works

</span>
6 0
3 years ago
What is "free" nitrogen?
alexandr1967 [171]

Answer:

d

Explanation:

soil need nutrient for it to help plant grow

5 0
3 years ago
Read 2 more answers
(fill in the blanks) In an ionic compound, the positive ion is called
klasskru [66]

Answer:

positive ion is a Cation while a negative ion is called an anion

7 0
3 years ago
If there are many forces acting on an object how can the net force be 0
zysi [14]
You have to balance out those forces and apply the same amount of equal and opposite force to it. I hope I helped ^^
4 0
3 years ago
Dissolving 5.28 g of an impure sample of calcium carbonate in hydrochloric acid produced 1.14 L of carbon dioxide at 20.0 °C and
swat32

Answer:

\%\ mass\ of\ CaCO_3=93.37\ \%

Explanation:

Given that:

Pressure = 791 mmHg

Temperature = 20.0°C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (20 + 273.15) K = 293.15 K  

T = 293.15 K  

Volume = 100 L

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 62.3637 L.mmHg/K.mol  

Applying the equation as:

791 mmHg × 1.14 L = n × 62.3637 L.mmHg/K.mol  × 293.15 K  

⇒n of CO_2 produced =  0.0493 moles

According to the reaction:-

CaCO_3 + 2 HCl\rightarrow CaCl_2 + H_2O + CO_2

1 mole of carbon dioxide is produced 1 mole of calcium carbonate reacts

0.0493 mole of carbon dioxide is produced 0.0493 mole of calcium carbonate reacts

Moles of calcium carbonate reacted = 0.0493 moles

Molar mass of CaCO_3 = 100.0869 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

0.0493\ mol= \frac{Mass}{100.0869\ g/mol}

Mass_{CaCO_3}=4.93\ g

Impure sample mass = 5.28 g

Percent mass is percentage by the mass of the compound present in the sample.

\%\ mass\ of\ CaCO_3=\frac{Mass_{CaCO_3}}{Total\ mass}\times 100

\%\ mass\ of\ CaCO_3=\frac{4.93}{5.28}\times 100

\%\ mass\ of\ CaCO_3=93.37\ \%

3 0
3 years ago
Other questions:
  • Please help. Last grade of this class
    5·1 answer
  • Water that is returned to the environment after secondary treatment is known as
    13·2 answers
  • You are writing a safety contract for your class. List 10 things you would include in the contract?
    14·2 answers
  • What do you think is meant by the term pseudoscience?
    13·2 answers
  • Explain sp hybridization in acetylene molecule? Dr
    10·1 answer
  • A substance absorbed 895 J and caused its temperature to increase by 10 ºC. If the substance has a mass of 27.9 g, what is the s
    10·2 answers
  • GIVING BRAILIEST FOR ANSWER
    5·2 answers
  • Which process is shown in the diagram?
    13·1 answer
  • What will the volume be of a soltuion created using 120 ml of 4.5 M stock solution if the final molarity needs to be 2.00 M
    12·1 answer
  • What type of elements form ionic bonds with metals
    10·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!