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3 years ago

11

A certain redox reaction takes place in a basic solution . which species must you include to balance the equation for this react

ion

2 answers:

Arte-miy333 [17]3 years ago

3 0

OH

*inserts random text so that this answer can be posted reaching the needed amount of words.*

Musya8 [376]3 years ago

3 0

The correct answer is OH

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How many grams are in 8.23 moles of sodium oxide?

konstantin123 [22]

Answer:

So, the mole ratio between sodium and sodium oxide is 2:1=2

Explanation:

6 0

2 years ago

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A compound contains only carbon, hydrogen, and oxygen. combustion of 11.75 mg of the compound yields 17.61 mg co2 and 4.81 mg h2

Ymorist [56]

Number of moles is defined as the ratio of given mass in g to the molar mass.

First, convert the given mass of carbon dioxide in mg to g:

1 mg = 0.001 g

17.61 mg = 0.01761 g

Number of moles of carbon dioxide = $\frac{0.01761 g}{44.01 g/mol}$

= $0.0004001 mol$

Mass of carbon = number of moles of carbon dioxide \times molar mass of carbon

= $0.0004001 mol\times 12.011 g/mol$

= $0.004806 g$

Number of moles of water= $\frac{0.00481 g}{18 g/mol}$

= $2.672\times 10^{-4}$

Since, water contains two hydrogen atoms. Thus,

Moles of hydrogen = $2\times 2.672\times 10^{-4}$

= $5.34\times 10^{-4}$

Mass of hydrogen = $5.34\times 10^{-4}\times \times 1.008 g/mol$

= $5.34\times 10^{-4} g$

Mass of oxygen = $0.001175-(5.38\times 10^{-4}g+0.004806 g)$

= $0.006405 g$

Number of moles of oxygen = $\frac{0.006405 g}{15.999 g/mol}$

= $0.000400$

Now,

$C_{0.0004001} H_{0.000534} O_{0.000400}$

Divide the smallest number to get the whole number,

$C_{\frac{0.0004001}{0.000400}} H_{\frac{0.000534}{0.000400}} O_{\frac{0.000400}{0.000400}}$

we get,

$C_{1} H_{1.33} O_{1}$

Now, multiply all the subscript by 3 to get the whole number,

$C_{3} H_{4} O_{3}$ (empirical fomula)

Molar mass of the compound = $3\times 12.011 g/mol+4\times 1.008 g/mol+3\times 15.999 g/mol$

= $88.062 g/mol$

Divide given molar mass of the compound with the molar mass of the compound.

= $\frac{176.1 g/mol}{88.062 g/mol}$

= $1.999\simeq 2$

Thus, multiply the subscripts of empirical formula by 2 to get the molecular formula, we get:

$C_{6}H_{8}O_{6}$

Hence, empirical formula is $C_{3}H_{4}O_{3}$ and molecular formula is $C_{6}H_{8}O_{6}$

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3 years ago

When calcium hydroxide powder is placed into a hydrochloric acid solution, aqueous calcium chloride and water are formed?

Vanyuwa [196]

<span>Answer: yes, when calcium hydroxide powder is placed into a hydrochloric acid solution, aqueous calcium hydroxide and water are formed.
</span>
<span /><span /><span>
Explanation:

</span><span>1) Calcium hydroxide is a base whose chemical formula is: Ca(OH)₂</span>
<span /><span>
2) Hydrochloric acid is the acid with chemical formula HCl

</span><span>3) Acids and bases react in a double replacement reaction forming salt plus water: Acid + Base → salt + water
</span>
<span /><span /><span>
4) The specific chemical equation for these reactants is:

</span><span>Ca(OH)₂ (s) + 2HCl(aq) → CaCl₂ (aq) + 2H₂O(l)</span>
<span /><span>
</span><span>5) CaCl₂ is calcium chloride, a salt, and H₂O is water
</span><span>
</span>

5 0

3 years ago

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Consider the reaction below. Which species are conjugate acid/base pairs? H2SO3 (aq) + CN (aq) HSO3 (aq)HCN (aq) A) HSO3, CN B)

SpyIntel [72]

Answer : The correct option is, (B) $H_2SO_3,HSO_3^-$

Explanation :

According to the Bronsted Lowry concept, Bronsted Lowry-acid is a substance that donates one or more hydrogen ion in a reaction and Bronsted Lowry-base is a substance that accepts one or more hydrogen ion in a reaction.

Or we can say that, conjugate acid is proton donor and conjugate base is proton acceptor.

The given equilibrium reaction is,

$H_2SO_3(aq)+CN^-\rightleftharpoons HSO_3^-(aq)+HCN(aq)$

Here, $H_2SO_3$ is loosing a proton, thus it is considered as an acid and after losing a proton, it forms $HSO_3^{-}$ which is a conjugate base. That means, $H_2SO_3/HSO_3^-$ are act as a conjugate acid-base pairs.

Hence, correct option is, (B) $H_2SO_3,HSO_3^-$

7 0

3 years ago

You have a 5-liter container with 2.00 x 10^23 molecules of ammonia gas (NH3) at STP. How many molecules of argon gas (Ar) are i

irga5000 [103]

Answer:

C. $2.00\times 10^{23}$ molecules

Explanation:

Since, the temperature, pressure and volume conditions are same, the molecules of ammonia gas must be equal to the molecules of the argon according to the ideal gas equation which is shown below 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 = 0.0821 L.atm/K.mol

Thus, both will have same moles and same number of molecules.

<u>Thus, molecules of argon = $2.00\times 10^{23}$ molecules</u>

8 0

3 years ago