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3 years ago

the actual yield of a certain reaction is 38.0 g while the theoretical yield is 50.0 g calculate the percent yield

Chemistry

1 answer:

Verizon [17]3 years ago

8 0

Answer:

76%

Explanation:

Actual yield = 38.0 g

Theoretical yield = 50.0 g

Percentage yield = ?

The relationship between these quantities is given as;

Percent yield = Actual yield / Theoretical yield * 100%

Percent yield = 38 g / 50 g * 100 %

Percent yield = 0.76 * 100 % = 76%

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6. If 4 mole of the rocket fuel ammonium perchlorate, NH4C/04 (s) is

Bond [772]

Answer:

144g of H₂O

Explanation:

3NH₄ClO₄(s) + 3Al → Al₂O₃(s) + AlCl₃(s) + 3NO(g) + 6H₂O(g)

From the equation:

3 moles of NH₄ClO₄ produced 6 moles of H₂O

4 moles of NH₄ClO₄ produced ? moles of H₂O

(4 ₓ 6)/3 = $\frac{24}{3}$ = 8 moles of H₂O

1 mole of H₂O = (1 × 2) + 16 = 18g (The Relative Molecular mass of H₂O)

8 moles of H₂O = ?

Therefore 8 × 18 = 144g

=144g of H₂O

3 0

2 years ago

What is the percentage yield of O2 if 12.3 g of KClO3 (molar mass 123 g) is decomposed to produce 3.2 g of O2 (molar mass 32 g)

My name is Ann [436]

Answer:

The percentage yield of O2 is 66.7%

Explanation:

Reaction for decomposition of potassium chlorate is:

2KClO₃ → 2KCl + 3O₂

The products are potassium chloride and oxygen.

Let's find out the moles of chlorate.

Mass / Molar mass = Moles

12.3 g / 123 g/mol = 0.1 mol

So ratio is 2:3, 2 moles of chlorate produce 3 mol of oxygen.

Then, 0.1 mol of chlorate may produce (0.1 .3)/ 2 = 0.15 moles

Let's convert the moles of produced oxygen, as to find out the theoretical yield.

0.15 mol . 32 g/ 1mol = 4.8 g

To calculate the percentage yield, the formula is

(Produced Yield / Theoretical yield) . 100 =

(3.2g / 4.8g) . 100 = 66.7 %

8 0

3 years ago

What is the result of having two batteries on an electric motor

aleksley [76]

Answer:

Well bro lemme tell u,

by connecting batteries, you can increase the voltage, amperage, or both.

Explanation:

8 0

2 years ago

Does pressure decrease when a gas is removed

vovangra [49]

yes

Explanation:

the volume also decrease. as particles are removed from the space the gas is in, there is a decrease in the number of collisions.

4 0

3 years ago

At 1.00 atmosphere pressure, a certain mass of a gas has a temperature of 100oC. What will be the temperature at 1.13 atmosphere

Inessa [10]

Answer: Final temperature of the gas will be 330 K.

Explanation:

Gay-Lussac's Law: This law states that pressure is directly proportional to the temperature of the gas at constant volume and number of moles.

$P\propto T$ (At constant volume and number of moles)

${P_1\times T_1}={P_2\times T_2}$

where,

$P_1$ = initial pressure of gas = 1.00 atm

$P_2$ = final pressure of gas = 1.13 atm

$T_1$ = initial temperature of gas = $100^0C=(100+273)K=373K$ K

$T_2$ = final temperature of gas = ?

${1.00\times 373}={1.13\times T_2}$

$T_2=330K$

Therefore, the final temperature of the gas will be 330 K.

7 0

3 years ago