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Rzqust [24]
2 years ago
7

How many grams of CaO can be produced using 3.9 moles CaCO3?1 CaCO3 --> 1CaO + 1CO *

Chemistry
1 answer:
Lina20 [59]2 years ago
4 0

Answer: 218.4 g of CaO will be produced from 3.9 moles of CaCO_3

Explanation:

The balanced chemical equation is:

CaCO_3\rightarrow CaO+CO_2  

According to stoichiometry :

1 mole of CaCO_3 produce =  1 mole of CaO

Thus 3.9 moles of CaCO_3 will produce=\frac{1}{1}\times 3.9=3.9moles of CaO

Mass of CaO=moles\times {\text {Molar mass}}=3.9moles\times 56g/mol=218.4g

Thus 218.4 g of CaO will be produced from 3.9 moles of CaCO_3

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Metallic properties tend to increase in which direction on the periodic table
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Metallic properties head to the left.
3 0
2 years ago
20cm of 0.09M solution of H2SO4. requires 30cm of NaOH for complete neutralization. Calculate the
kirill115 [55]

Answer:

Choice A: approximately 0.12\; \rm M.

Explanation:

Note that the unit of concentration, \rm M, typically refers to moles per liter (that is: 1\; \rm M = 1\; \rm mol\cdot L^{-1}.)

On the other hand, the volume of the two solutions in this question are apparently given in \rm cm^3, which is the same as \rm mL (that is: 1\; \rm cm^{3} = 1\; \rm mL.) Convert the unit of volume to liters:

  • V(\mathrm{H_2SO_4}) = 20\; \rm cm^{3} = 20 \times 10^{-3}\; \rm L = 0.02\; \rm L.
  • V(\mathrm{NaOH}) = 30\; \rm cm^{3} = 30 \times 10^{-3}\; \rm L = 0.03\; \rm L.

Calculate the number of moles of \rm H_2SO_4 formula units in that 0.02\; \rm L of the 0.09\; \rm M solution:

\begin{aligned}n(\mathrm{H_2SO_4}) &= c(\mathrm{H_2SO_4}) \cdot V(\mathrm{H_2SO_4})\\ &= 0.02 \; \rm L \times 0.09 \; \rm mol\cdot L^{-1} = 0.0018\; \rm mol \end{aligned}.

Note that \rm H_2SO_4 (sulfuric acid) is a diprotic acid. When one mole of \rm H_2SO_4 completely dissolves in water, two moles of \rm H^{+} ions will be released.

On the other hand, \rm NaOH (sodium hydroxide) is a monoprotic base. When one mole of \rm NaOH formula units completely dissolve in water, only one mole of \rm OH^{-} ions will be released.

\rm H^{+} ions and \rm OH^{-} ions neutralize each other at a one-to-one ratio. Therefore, when one mole of the diprotic acid \rm H_2SO_4 dissolves in water completely, it will take two moles of \rm OH^{-} to neutralize that two moles of \rm H^{+} produced. On the other hand, two moles formula units of the monoprotic base \rm NaOH will be required to produce that two moles of \rm OH^{-}. Therefore, \rm NaOH and \rm H_2SO_4 formula units would neutralize each other at a two-to-one ratio.

\rm H_2SO_4 + 2\; NaOH \to Na_2SO_4 + 2\; H_2O.

\displaystyle \frac{n(\mathrm{NaOH})}{n(\mathrm{H_2SO_4})} = \frac{2}{1} = 2.

Previous calculations show that 0.0018\; \rm mol of \rm H_2SO_4 was produced. Calculate the number of moles of \rm NaOH formula units required to neutralize that

\begin{aligned}n(\mathrm{NaOH}) &= \frac{n(\mathrm{NaOH})}{n(\mathrm{H_2SO_4})}\cdot n(\mathrm{H_2SO_4}) \\&= 2 \times 0.0018\; \rm mol = 0.0036\; \rm mol\end{aligned}.

Calculate the concentration of a 0.03\; \rm L solution that contains exactly 0.0036\; \rm mol of \rm NaOH formula units:

\begin{aligned}c(\mathrm{NaOH}) &= \frac{n(\mathrm{NaOH})}{V(\mathrm{NaOH})} = \frac{0.0036\; \rm mol}{0.03\; \rm L} = 0.12\; \rm mol \cdot L^{-1}\end{aligned}.

3 0
3 years ago
What is the coefficient for oh−(aq) when s2−(aq) no3−(aq) → s(s) no(g) is balanced in basic aqueous solution?
omeli [17]

From the balanced redox equation of the reaction, the coefficient of OH⁻ is 8.

<h3>What is the balanced redox equation of the reaction?</h3>

A redox equation is the equation of a redox reaction in which oxidation and reduction occurs simultaneously.

The given redox reaction takes place in a basic solution

The balanced redox equation of the reaction is given below:

4 H₂O(l) + 3 S²⁻(aq) + 2 NO₃⁻(aq) ---> 3 S(s) + 2 NO + 8 OH⁻(aq)

In conclusion, a redox equation is balanced when oxidation and reduction occur to the same extent.

Learn more about redox equations at: brainly.com/question/26750732

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5 0
1 year ago
A chemical company makes two brands of antifreeze. the first brand is 70% pure antifreeze, and the second brand is 95% pure anti
madreJ [45]

Answer is: 56 gallons of 70% antifreeze and 84 gallons of 95% antifreeze.


ω₁ = 70% ÷ 100% = 0.7; 70% pure antifreeze.

ω₂ = 95% ÷ 100% = 0.95.

ω₃<span> = 85% ÷ 100% = 0.85.
V</span>₁ = ?; volume of 70% antifreeze.

V₂ = ?; volume of 95% antifreeze.<span>
V</span>₃ = V₁ + V₂<span>.
V</span>₃ = 140 gal.

V₁ = 140 gal - V₂<span>.
ω</span>₁ · V₁ + ω₂ ·V₂ = ω₃ · V₃.

0.70 · (140 gal - V₂) + 0.95 · V₂ = 0.85 · 140 gal.

98 gal - 0.7V₂ + 0.95V₂ = 119 gal.

0.25V₂ = 21 gal.

V₂ = 21 gal ÷ 0.25.

V₂ = 84 gal.

V₁ = 140 gal - 84 gal.

V₁ = 56 gal.

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