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3 years ago

Using stoichiometry, you predict that you should be able to use 314.0 g of Al to produce 1551 g of AlCi3. In your lab

Chemistry

1 answer:

Alex787 [66]3 years ago

6 0

Answer:

90.26%

Explanation:

From the question given above, the following data were obtained:

Theoretical yield of AlCl₃ = 1551 g

Actual yield of AlCl₃ = 1400 g

Percentage yield =?

The percentage yield of the reaction can be obtained as follow:

Percentage yield = Actual yield / Theoretical yield × 100

Percentage yield = 1400 / 1551 × 100

Percentage yield = 140000 / 1551

Percentage yield = 90.26%

Thus, the percentage yield of the reaction is 90.26%

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4 years ago

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3 years ago

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3 years ago

At equilibrium, a 1.00 M OClÈ solution has an [OHÈ] of 5.75 × 10ÈÊ M. Which of the following is the correct pH of the solution?

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3 0

3 years ago

In the laboratory a student determines the specific heat of a metal. He heats 19.5 grams of copper to 98.27 °C and then drops it

siniylev [52]

Answer:

The specific heat of copper is 0.37 J/g°C

Explanation:

Step 1: Data given

Mass of copper = 19.5 grams

Initial temperature of copper = 98.27 °C

Mass of water = 76.3 grams

Initial temperature of water = 24.05 °C

Final temperature of water and copper = 25.69 °C

Step 2: Calculate specific heat of copper

Qgained = -Qlost

Q = m*c*ΔT

Qwater = -Qcopper

m(water) * c(water) * ΔT(water) = - m(copper) * c(copper) *ΔT(copper)

⇒ with m(water) = 76.3 grams

⇒ with c(water) = 4.184 J/g°C

⇒ with ΔT(water) = T2-T1 = 25.69 - 24.05 = 1.64

⇒ with m(copper) = 19.5 grams

⇒ with c(copper) = TO BE DETERMINED

⇒ with ΔT(copper) = T2-T1 = 25.69 - 98.27 = -72.58

76.3 * 4.184 * 1.64 = - 19.5 * c(copper) * -72.58

523.552 = 1415.31 * c(copper)

c(copper) = 0.37 J/g°C

The specific heat of copper is 0.37 J/g°C

3 0

4 years ago