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lianna [129]
2 years ago
6

Bohr's Model of the atom

Chemistry
1 answer:
AlexFokin [52]2 years ago
3 0

Answer:

group 17 the halogen.as it has 7 electron in its outermost ring

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What is the predicted outcome for very low mass stars (those that are smaller than about the mass of the sun)?
White raven [17]

Answer:

In case of low-mass stars,the outer layers of the low mass stars are expelled  as the core collapses such that the outer layers form a planetary nebula.

Explanation:

In case of low-mass stars,the outer layers of the low mass stars are expelled  as the core collapses such that the outer layers form a planetary nebula. The core remains as a white dwarf and finally become a black dwarf as it cools down. A low mass star consumes its core hydrogen and turns it into helium over its lifetime.

4 0
2 years ago
During an endothermic phase change, what happens to the potential energy and the kinetic energy?
Dovator [93]
The correct answer should be that Potential energy increases, and kinetic energy increases, since they both increase as the temperature changes.
7 0
2 years ago
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Urea, (NH2)2CO, is a product of metabolism of proteins. An aqueous solution is 37.2% urea by mass and has a density of 1.032 g/m
Feliz [49]

Answer:

The molarity of urea in this solution is 6.39 M.

Explanation:

Molarity (M) is <em>the number of moles of solute in 1 L of solution</em>;  that is

molarity = moles of solute ÷ liters of solution

To calculate the molality, we need to know the number of moles of urea and the volume of solution in liters. We assume 100 grams of solution.

Our first step is to calculate the moles of urea in 100 grams of the solution,

using the molar mass a conversion factor. The total moles of 100g of a 37.2 percent by mass solution is

60.06 g/mol ÷ 37.2 g = 0.619 mol

Now we need to calculate the volume of 100 grams of solution, and we use density as a conversion factor.

1.032 g/mL ÷ 100 g = 96.9 mL

This solution contains 0.619 moles of urea in 96.9 mL of solution. To express it in molarity, we need to calculate the moles present in 1000 mL (1 L) of the solution.

0.619 mol/96.9 mL × 1000 mL= 6.39 M

Therefore, the molarity of the solution is 6.39 M.

4 0
3 years ago
How many moles are in 25 grams of dihydrogen monoxide
timurjin [86]
If you'd like the full working, here it is:

I calculated this by using the formula triangle.

Mass

Number Formula
Of moles Mass

To calculate the number if moles in a substance, you need to divide the Mass by the Formula mass. You get the formula mass by adding the atomic masses of the elements in the compound together. In this situation, H2O, it would be two hydrogen molecules plus one oxygen molecule which is 2 + 16. This is because the atomic mass of Hydrogen is 1 and the atomic mass of Oxygen is 16.

Now that we have the Formula mass we can go ahead and do the calculation since we already have the Mass. You do as follows:

Mass divided by Formula mass which is in this case - 25 divided by 18

By doing this calculation you will get the answer which is 1.38 moles which can be rounded to 1.4

Hope this helps :)
6 0
3 years ago
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What is true about energy in an ordinary chemical reaction? Energy is
Lisa [10]
The answer is statement #3.
4 0
3 years ago
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