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2 years ago

6

What is the percent by mass of calcium in calcium carbonate,

1 answer:

motikmotik2 years ago

5 0

What is the percent by mass of calcium in calcium carbonate, CaCO3? (Molar mass of CaCO3 = 100.09 g/mol)

Answer: 40.04 percent

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Which model uses nuclear fusion Thomason model or the Bohr model (it’s the second bullet point)

Diano4ka-milaya [45]

Answer:

Aye bro you from discovery too

Explanation:

8 0

2 years ago

Balance the following redox equation using the smallest integers possible and select the correct coefficient for the hydrogen su

goldfiish [28.3K]

Answer:

Coefficient of $HSO_{3}^{-}$ is 5

Explanation:

Oxidation: $MnO_{4}^{-}(aq)\rightarrow Mn^{2+}(aq)$

Balance O and H in acidic medium: $MnO_{4}^{-}(aq)+8H^{+}(aq)\rightarrow Mn^{2+}(aq)+4H_{2}O(l)$
Balance charge : $MnO_{4}^{-}(aq)+8H^{+}(aq)+5e^{-}\rightarrow Mn^{2+}(aq)+4H_{2}O(l)$ .............(1)

Reduction: $HSO_{3}^{-}\rightarrow SO_{4}^{2-}$

Balance O and H in acidic medium : $HSO_{3}^{-}(aq)+H_{2}O(l)\rightarrow SO_{4}^{2-}(aq)+3H^{+}(aq)$
Balance charge : $HSO_{3}^{-}(aq)+H_{2}O(l)-2e^{-}\rightarrow SO_{4}^{2-}(aq)+3H^{+}(aq)$ ..............(2)

$[2\times eq(1)]+[5\times eq(2)]$ -

Balanced equation: $2MnO_{4}^{-}(aq)+5HSO_{3}^{-}(aq)+H^{+}(aq)\rightarrow 2Mn^{2+}(aq)+5SO_{4}^{2-}(aq)+3H_{2}O(l)$

Coefficient of $HSO_{3}^{-}$ is 5

8 0

2 years ago

A canoe displaces 100 L of water. Water weighs 9.8 N/L. What is the buoyant force on the canoe?

Setler79 [48]

Hey there!

The Buoyant force is going to be equal to the weight of the water displaced and it would be like this 100 L(9.8 N/L) = 980 N.

Hope this helped and mind marking me brainliest. Thank you!

5 0

3 years ago

Read 2 more answers

What will happen if a large quantity of NaCl is added to the aqueous solution?

vlabodo [156]

It will explode...............

5 0

2 years ago

Read 2 more answers

A 2.89 g sample of a metal chloride, MCl2, is dissolved in water and treated with excess aqueous silver nitrate. The silver chlo

dsp73

Answer:

58.0 g/mol

Explanation:

The reaction that takes place is:

MCl₂ + 2AgNO₃ → 2AgCl + M(NO₃)₂

First we <u>calculate how many moles of silver chloride</u> were produced, using its <em>molar mass</em>:

6.41 g AgCl ÷ 143.32 g/mol = 0.0447 mol AgCl

Then we <u>convert AgCl moles into MCl₂ moles</u>, using the <em>stoichiometric ratio</em>:

0.0447 mol AgCl * $\frac{1molMCl_2}{2molAgCl}$ = 0.0224 mol MCl₂

Now we<u> calculate the molar mass of MCl₂</u>, using the original<em> mass of the sample</em>:

2.86 g / 0.0224 mol = 127.68 g/mol

We can write the molar mass of MCl₂ as:

Molar Mass MCl₂ = Molar Mass of M + (Molar Mass of Cl)*2

127.68 g/mol = Molar Mass of M + (35.45 g/mol)*2

Finally we<u> calculate the molar mass</u> of M:

Molar Mass of M = 57 g/mol

The closest option is 58.0 g/mol.

6 0

3 years ago