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
Gelneren [198K]
3 years ago
7

You carefully weigh out 13.00 g of CaCO3 powder and add it to 52.65 g of HCl solution. You notice bubbles as a reaction takes pl

ace. You then weigh the resulting solution and find that it has a mass of 60.32
g. The relevant equation isCaCO3(s)+2HCl(aq)?H2O(l)+CO2(
g.+CaCl2(aq)Assuming no other reactions take place, what mass of CO2 was produced in this reaction?Express your answer to three significant figures and include the appropriate units.
Chemistry
2 answers:
Sedbober [7]3 years ago
7 0
CaCO₃ + 2HCl = CaCl₂ + CO₂ + H₂O

n(CaCO₃)=m(CaCO₃)/M(CaCO₃)
n(CaCO₃)=13.00/100.09=0.1299 mol

Δm=13.00+52.65-60.32=5.33 g

m(CO₂)=5.33 g
n(CO₂)=5.33/44.01=0,1211 mol

w=0.1211/0.1299=0,9323 (93.23%)

rosijanka [135]3 years ago
7 0

Answer:

The amount of carbon dioxide produced is 5.33 gr.

Explanation:

The easiest way to solve this problem it by knowing that the mass of a sistem is always the same (the mass can't be created or destroyed, only converted).

Following that statement, we can substract from the final mass of the reaction (60.32gr), the mass of the reactives (13 gr and 52.65 gr), and keeping in mind that the only mass that can't be weight is the mass of CO₂ because it leaves the sistem in the form of a gas:

Δm = 60.32-13.00-52.65=-5.33 g

The negative indicates a lack of mass, in this case the CO₂  wich has been produced.

If we look at the reaction equation, we can see that for each mol of CaCO₃, it is produced one mol of CO₂.

CaCO₃ + 2HCl = CaCl₂ + CO₂ + H₂O

Knowing the amount of CaCO₃ (13 gr) and  searching in the periodic table to  find its molar mass, we can say that we have 0.12988 mol of CaCO₃.

Doing the same steps for carbon dioxide, we can see that only 0.1211  mol of CO₂ have been produced. That indicates that te reaction has not been completed.

You might be interested in
Write a balanced chemical equation describing the oxidation of the bromide ion by solid xenon trioxide to produce bromine liquid
ki77a [65]

Answer:

6Br⁻ + XeO₃ + 6H⁺ → 3Br₂ + Xe + 3H₂O  

Explanation:

First, we need to write the half-reactions:

2Br⁻ → Br₂ + 2e⁻ Oxidation -Balanced yet-

XeO₃ →  Xe Reduction

To balance the reduction in acidic aqueous solution we need to add waters in the other side of the reaction as oxygens are present:

XeO₃ →  Xe + 3H₂O

And H⁺ as hydrogens from water we have:

XeO₃ + 6H⁺ →  Xe + 3H₂O

To balance the charge:

<h3>XeO₃ + 6H⁺ + 6e⁻ →  Xe + 3H₂O  Reduction -Balanced-</h3><h3 />

To cancel out the electrons of both half-reaction we need to multiply oxidation 3 times:

6Br⁻ → 3Br₂ + 6e⁻

XeO₃ + 6H⁺ + 6e⁻ →  Xe + 3H₂O  

And the balanced reaction in acidic aqueous solution is the sum of both half-reactions:

<h3>6Br⁻ + XeO₃ + 6H⁺ → 3Br₂ + Xe + 3H₂O  </h3>
5 0
2 years ago
Help!! Hurry!! I will mark brainliest if you get it correct. NO SPAM!!!!!!
Lelechka [254]

Answer:

216/84 Po + 4/2 He a

Explanation:

6 0
2 years ago
Read 2 more answers
How much heat is released when 105 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 4
Yuki888 [10]
1) (Hvap)(moles of water)=236.9783574kJ
(40.67)(105/18.02)
2) (change in temperature)(mass)(Cliquid)=43.9345172kJ
(100)(105/18.02)(75.4)/1000
3) (Hfus)(moles of water)=35.01942286kJ
(6.01)(105/18.02)
4) (change in temperature)(mass)(Csolid)=3.181465039kJ
(15)(105/18.02)(36.4)/1000
Total released=319.1137625kJ
5 0
3 years ago
2C₂H6 + 702 —&gt;4C02 + 6H₂O
navik [9.2K]

Answer:

975.56×10²³ molecules

Explanation:

Given data:

Number of molecules of C₂H₆ = 4.88×10²⁵

Number of molecules of CO₂ produced  =  ?

Solution:

Chemical equation:

2C₂H₆  + 7O₂     →      4CO₂ + 6H₂O

Number of moles of C₂H₆:

1 mole = 6.022×10²³ molecules

4.88×10²⁵  molecules×1mol/6.022×10²³ molecules

0.81×10² mol

81 mol

Now we will compare the moles of C₂H₆ with CO₂.

                     C₂H₆          :             CO₂

                          2           :               4

                           81         :           4/2×81 = 162 mol

Number of molecules of CO₂:

1 mole = 6.022×10²³ molecules

162 mol ×6.022×10²³ molecules / 1 mol

975.56×10²³ molecules

8 0
3 years ago
PLEASE ANSWER: The density of a gas at STP is 0.75 g/L. What is the mass of this gas?
BartSMP [9]

Answer:

the mass of the glass is 2

3 0
3 years ago
Other questions:
  • A bathtub is filled with 100 L of water. A cat jumps in and the volume rises to 125 L. If the cat has a mass of
    15·1 answer
  • How do the atoms that make up matter affect its characteristics and behavior?
    14·1 answer
  • What is the [pb2+] in a solution made by adding 100 g of pbcl2(s) (mm = 278.1 g/mol) to a 5.4 m solution of nacl and allowing it
    5·1 answer
  • How are atomic mass and mass number similar
    14·1 answer
  • Where does Ta, Os, Rh comes from?
    12·1 answer
  • Which of the following best describes the relationship between products and reactants in an exothermic reaction?
    6·2 answers
  • A new radio station, KHEM-AM, broadcasts
    9·1 answer
  • 24 g of magnesium to mol
    13·1 answer
  • Methane gas is collected over water at 25 C and an atmospheric pressure of 775 mmHg. What is the dry pressure of the gas at this
    13·1 answer
  • How many grams of C8H18<br> is in 405,576.398 mL
    8·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!