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olganol [36]
2 years ago
15

If the reaction described by this chemical equation started with 5.77 grams of PbO2 and resulted in 0.331 grams of O2, what is t

he percent yield of O2
Chemistry
1 answer:
____ [38]2 years ago
6 0

Answer:

42.9%

Explanation:

Step 1: Write the balanced decomposition reaction

PbO₂ ⇒ Pb + O₂

Step 2: Calculate the theoretical yield of O₂ from 5.77 g of PbO₂

According to the balanced equation, the mass ratio of PbO₂ to O₂ is 239.2:32.00.

5.77 g PbO₂ × 32.00 g O₂/239.2 g PbO₂ = 0.772 g O₂

Step 3: Calculate the percent yield of O₂

The real yield of O₂ is 0.331 g. The percent yield of O₂ is:

%yield = real yield / theoretical yield × 100%

%yield = 0.331 g / 0.772 g × 100% = 42.9%

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What is the relationship between elements ,atoms ,and compounds
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A total of 20.0 mL of sodium hydroxide (NaOH) was neutralized by 30.0 mL of 0.250 M hydrogen bromide (HBr). What was the concent
Karolina [17]

Answer:

0.375 M

Explanation:

NaOH(aq) + HBr(aq) ------------> NaBr(aq) + H2O(l)

Concetration of acid CA= 0.250M

Concentration of base CB= ????

Volume of acid VA= 30.0mL

Volume of base VB= 20.0mL

Number of moles of acid nA= 1

Number of moles of base nB= 1

CA VA/CB VB= nA/nB

CB= CAVAnB/VB nA

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8 0
3 years ago
What will happen to the pressure when the temperature of a gas increases
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For the chemical reaction
kakasveta [241]

Answer:

Mass = 199.21 g

Explanation:

Given data:

Moles of HCl = 3.59 mol

Mass of CaCl₂ = ?

Solution:

Chemical equation:

2HCl + Ca(OH)₂  →     CaCl₂ + 2H₂O

we will compare the moles of HCl with  CaCl₂ from balanced chemical equation:

                HCl             :           CaCl₂

                   2              :              1

                 3.59           :             1/2×3.59 = 1.795  

3.59 moles of HCl will produced 1.795 moles of CaCl₂.

Mass of CaCl₂.

Mass = number of moles × molar mass

Mass = 1.795 mol  × 110.98 g/mol

Mass = 199.21 g

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3 years ago
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