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
ch4aika [34]
3 years ago
11

When heated a sample consisting of only CaCO3 and MgCO3 yields a mixture of CaO and Mgo. If the weight of the combined oxides is

equal to 51.00% of the initial sample weight, calculate the per cent of CaCO3 and MgCO3 in the sample. (12 M.)
Chemistry
1 answer:
ExtremeBDS [4]3 years ago
7 0

Answer:

38.83 %  of  CaCO3

61.17 %  of  MgCO3

Explanation:

where Moles of CaCO3 is equals to x and MgCO3 is y we have that...

CaCO3 molar mass = 100.09 g / mol  = 100.09 x

MgCO3 molar mass = 84.31 g / mol  = 84.31 y

decomposition reactions :

CaCO3 ---> CaO + CO2

MgCO3 ---> MgO + CO2  

So we have that , Moles of CaO = Moles of CaCO3 = x

and Moles of MgO = Moles of MgCO3 = y

CaO molar mass = 56.08 g / mol

MgO molar mass = 40.30 g / mol

CaO = 56.08 x

 MgO = 40.30 y

"If the weight of the combined oxides is equal to 51.00% of the initial sample weight,"

total mass of MgO and CaO = 51.00 % of Total Mass of MgCO3 and CaCO3  

thus

56.08 x + 40.30 y = 0.51 ( 100.09 x + 84.31 y )

56.08 x + 40.30 y = 51.04 x + 42.99y

5.04 x = 2.7 y

y = 1.87 x    

CaCO3 % in the sample

= 100.09 x × 100 / ( 100.09 x + 84.31 y )

= 10009 x / ( 100.09 x + 84.31 × 1.87 x )

= 10009 x / ( x ( 100.09 + 157.66 ) )

= 10009 / 257.75

= 38.83 %

MgCO3 % in the sample

= 100 - 38.83  

=   61.17 %  

You might be interested in
A calorimeter contains 22.0 mL of water at 14.0 ∘C . When 2.50 g of X (a substance with a molar mass of 82.0 g/mol ) is added, i
Alik [6]

Answer:

The enthalpy change in the the reaction is -47.014 kJ/mol.

Explanation:

X(s)+H_2O(l)\rightarrow X(aq)

Volume of water in calorimeter = 22.0 mL

Density of water = 1.00 g/mL

Mass of the water in calorimeter = m

m=1.00 g/mL\times 22.0 mL=22 g

Mass of substance X = 2.50 g

Mass of the solution = M = 2.50 g + 22 g = 24.50 g

Heat released during the reaction be Q

Change in temperature =ΔT = 28.0°C - 14.0°C = 14.0°C

Specific heat of the solution is equal to that of water :

c = 4.18J/(g°C)

Q=Mc\times \Delta T

Q=24.50 g\times 4.18 J/g ^oC\times 14.0^oC=1,433.74 J=1.433 kJ

Heat released during the reaction is equal to the heat absorbed by the water or solution.

Heat released during the reaction =-1.433 kJ

Moles of substance X= \frac{2.50 g}{82.0 g/mol}=0.03048 mol

The enthalpy change, ΔH, for this reaction per mole of X:

\Delta H=\frac{-1.433 kJ}{0.03048 mol}=-47.014 kJ/mol

5 0
2 years ago
5. for the following measurements is expressed to three significant figures? a) 0.007 m b) 7077 mg c) 7.30 x 10^-7 km d) 0.070
Maksim231197 [3]
The answer is c
a) 1 sf
b) 4 sf
d) 2 sf
6 0
3 years ago
A short chain of monomer liquid not long enough to be considered a polymer is called a(n)?
Lady_Fox [76]

Answer:

d. oligomer it is the correct answer also if you would just search that up it pops up

7 0
2 years ago
The atomic number of an atom is
frosja888 [35]

Answer:

b, the number of protons added to the number of neutrons

Explanation:

5 0
3 years ago
300 grams of a compound which contains only carbon, hydrogen and oxygen is analyzed and found to contain the exact same percenta
ser-zykov [4K]

The empirical formula of the compound is C₄H₅O₃.

<u>Explanation</u>:

If hydrogen % = 5.98823, the Sum of C+O = 94.01177% or 47.005885% each

The original mass of 300 g is not important

C = 47.005885 / 12.011 = 3.913569

H = 5.98823 / 1.008 = 5.94070  

O = 47.005885 / 15.999 = 2.93805  

Divide by the smallest number:      

C =1.33  

H = 2.022

O = 1

Multiply through by 3

C = 4

H =6

O = 3

The empirical formula of a compound = C₄H₆O₃

Do not be confused by the 300 g. It is totally irrelevant to the question because you are dealing with % amounts. It would only have been of importance if you were given some mass values.

4 0
3 years ago
Other questions:
  • How to solve this problem given?
    14·1 answer
  • List four examples of diffusion seen in daily life.
    15·1 answer
  • Given the chemical equation: Fe2O3 + 3CO --&gt; 2Fe + 3CO2
    7·1 answer
  • If 5.100 g of c6h6 is burned and the heat produced from the burning is added to 5691 g of water at 21 °c, what is the final temp
    10·1 answer
  • Anyone Free can help me with this question please ?
    10·1 answer
  • Using the balanced chemical equation below. 2Al2O3 --&gt; 4Al + 3O2 How many moles of oxygen are produced if 11.0 mol of Al are
    6·1 answer
  • NEED HELP ASPA WILL MAKE THE BRAINIEST ANSWER
    14·1 answer
  • PLSS HELP!! BRAINILIST WILL BE GIVEN!!
    7·1 answer
  • Which of the following happens when an ionic bond is formed? (1 point)
    6·1 answer
  • When 20 ml of 0.1 M HCl is mixed with 20
    9·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!