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4 years ago

Which of these actions a sustainable practice?

Chemistry

1 answer:

tia_tia [17]4 years ago

8 0

<h2>Hello!</h2>

A sustainable practice is B. Setting usage limits on a resource

Sustainable practices are those that aim to reach an equilibrium between the use of natural resources for human development, and the preservation of the environment for future generations.

Setting usage limits on a resource is a sustainable practice because it allows for taking advantage of the resource, while providing constraints to its use, forcing the industry to be creative and develop alternative methods that take better advantage of that resource, or that use different resources (e.g. limiting fossil fuel emissions, forcing the industry to find alternative ways to generate power like solar energy).

Have a nice day!

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How many moles of oxygen are necessary to completely react with propane (C3H8) to produce 16.3 mol of water according to the fol

velikii [3]

The balanced chemical reaction is expressed as:

C3H8 + 5 O2 -> 3 CO2 + 4 H2O

We are given the amount of water produced. We use this amount for the calculations. We do as follows:

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Hope this answers the question. Have a nice day.

4 0

4 years ago

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If 500.0 mL of 0.10 M Ca2+ is mixed with 500.0 mL of 0.10 M SO42−, what mass of calcium sulfate will precipitate? Ksp for CaSO4

statuscvo [17]

Answer:

The mass of calcium sulfate that will precipitate is 6.14 grams

Explanation:

Step 1: Data given

500.0 mL of 0.10 M Ca^2+ is mixed with 500.0 mL of 0.10 M SO4^2−

Ksp for CaSO4 is 2.40*10^−5

Step 2: Calculate moles of Ca^2+

Moles of Ca^2+ = Molarity Ca^2+ * volume

Moles of Ca^2+ = 0.10 * 0.500 L

Moles Ca^2+ = 0.05 moles

Step 3: Calculate moles of SO4^2-

Moles of SO4^2- = 0.10 * 0.500 L

Moles SO4^2- = 0.05 moles

Step 4: Calculate total volume

500.0 mL + 500.0 mL = 1000 mL = 1L

Step 5: Calculate Q

Q = [Ca2+] [SO42-]

[Ca2+]= 0.050 M [O42-]

Qsp = (0.050)(0.050 )=0.0025 >> Ksp

This means precipitation will occur

Step 6: Calculate molar solubility

Ksp = 2.40 * 10^-5 = [Ca2+][SO42-] =(x)(x)

2.40 * 10^-5 = x²

x = √(2.40 * 10^-5)

x = 0.0049 M = Molar solubility

Step 7: Calculate total CaSO4 dissolved

total CaSO4 dissolved = 0.0049 M * 1 L * 136.14 mol/L = 0.667 g

Step 8: Calculate initial mass of CaSO4

Since initial moles CaSo4 = 0.050

Initial mass of CaSO4 = 0.050 * 136.14 g/mol

Initial mass of CaSO4 = 6.807 grams

Step 9: Calculate mass precipitate

6.807 - 0.667 = 6.14 grams

The mass of calcium sulfate that will precipitate is 6.14 grams

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