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3 years ago

Water molecules form hydrogen bonds to help in the process of water transport. Which property of water is described?

1 answer:

7 0

The property of water which is described in the lines above is cohesion.
It refers to the fact that water molecules stick to other water molecules, i. e. to themselves, as opposed to sticking to another material, which happens with adhesion. Water and capillaries don't have any connection.

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What are some questions you would ask to learn more about the toxic algal bloom in Lake Temescal? Include at least two questions

Darina [25.2K]

Answer:

How can we prevent harmful algae blooms?

How do you know if algal blooms are harmful?

Explanation:

I hope this helps

5 0

3 years ago

When 1.00 g of boron is burned in o2(g) to form b2o3(s), enough heat is generated to raise the temperature of 733 g of water fro

Bas_tet [7]

Answer: For this problem, you would need to know the specific heat of water, that is, the amount of energy required to raise the temperature of 1 g of water by 1 degree C. The formula is q = c X m X delta T, where q is the specific heat of water, m is the mass and delta T is the change in temperature. If we look up the specific heat of water, we find it is 4.184 J/(g X degree C). The temperature of the water went up 20 degrees. 4.184 x 713 x 20.0 = 59700 J to 3 significant digits, or 59.7 kJ. Now, that is the energy to form B2O3 from 1 gram of boron. If we want kJ/mole, we need to do a little more work. To find the number of moles of Boron contained in 1 gram, we need to know the gram atomic mass of Boron, which is 10.811. Dividing 1 gram of boron by 10.811 gives us .0925 moles of boron. Since it takes 2 moles of boron to make 1 mole B2O3, we would divide the number of moles of boron by two to get the number of moles of B2O3. .0925/2 = .0462 moles...so you would divide the energy in KJ by the number of moles to get KJ/mole. 59.7/.0462 = 1290 KJ/mole.

7 0

4 years ago

Combining hydrogen and oxygen to make water is a physical change

shutvik [7]

id say physical cause your changing the physical form of the molucles

3 0

3 years ago

A _____ is an experimental set-up that can be used to measure the heat of a chemical reaction or a physical change and determine

Eduardwww [97]

Answer:Calorimetry

Explanation: In this case, an instrument called Calorimeter is used to measure the amount of heat being transferred

7 0

3 years ago

If 6.00 g of CaCl2 • 2 H2O and 5.50 g of Na2CO3 are allowed to react in aqueous solution, what mass of CaCO3 will be produced? P

Andre45 [30]

Answer:

6.00 g CaCl₂ .2H₂O /1 × 1 mol CaCl₂ .2H₂O / 147 g CaCl₂ .2H₂O × 0.04 mol CaCO₃/ 0.04 mol of CaCl₂ .2H₂O × 100 g CaCO₃ / 1 mole CaCO₃ = 4 g

5.50 g Na₂CO₃ /1 × 1 Na₂CO₃ / 106 g Na₂CO₃ × 0.05 mol CaCO₃/ 0.05 mol of Na₂CO₃ × 100 g CaCO₃ / 1 mole CaCO₃ = 5 g

Explanation:

Given data:

Mass of CaCl₂.2H₂O = 6.00 g

Mass of Na₂CO₃ = 5.50 g

Mass of CaCO₃ produced = ?

Solution:

Number of moles of CaCl₂.2H₂O.

Number of moles = mass/ molar mass

Number of moles = 6.00 g/ 147 g/ mol

Number of moles = 0.04 mol

Number of moles of Na₂CO₃:

Number of moles = mass/ molar mass

Number of moles = 5.50 g/ 106 g/ mol

Number of moles = 0.05 mol

Chemical equation:

CaCl₂ + Na₂CO₃ → CaCO₃ + 2NaCl

Now we will compare the moles of CaCO₃ with Na₂CO₃ and CaCl₂ through balanced chemical equation .

CaCl₂ : CaCO₃

1 : 1

0.04 : 0.04

Mass of CaCO₃:

Mass = number of moles × molar mass

Mass = 0.04 mol× 100 g/mol

Mass = 4 g

6.00 g CaCl₂ .2H₂O /1 × 1 mol CaCl₂ .2H₂O / 147 g CaCl₂ .2H₂O × 0.04 mol CaCO₃/ 0.04 mol of CaCl₂ .2H₂O × 100 g CaCO₃ / 1 mole CaCO₃ = 4 g

Na₂CO₃ : CaCO₃

1 : 1

0.05 : 0.05

Mass of CaCO₃:

Mass = number of moles × molar mass

Mass = 0.05 mol× 100 g/mol

Mass = 5 g

5.50 g Na₂CO₃ /1 × 1 Na₂CO₃ / 106 g Na₂CO₃ × 0.05 mol CaCO₃/ 0.05 mol of Na₂CO₃ × 100 g CaCO₃ / 1 mole CaCO₃ = 5 g

5 0

3 years ago