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2 years ago

GIVING 17 POINTS PLS HELP ME!!!!

1 answer:

8 0

Hydropower can affect fish and other marine life which is the true statement and is denoted as option C.

<h3>What is Hydropower?</h3>

This is the process in which water energy is converted into electrical energy through the use of dams and turbines.

When the dams are created, it blocks the path of marine activities and limits them to certain activities such as reproduction.

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How to find the oxidation number of an element

Virty [35]

The thing you MUST do FIRST is look for any H's, O's, or F's in the equation

1)any element just by itself not in a compound, their oxidation number is 0
ex: H2's oxidation number is 0
ex: Ag: oxidation number is 0 if its just something like Ag + BLA = LALA

2) the oxidation number of H is always +1, unless its just by itself (see #1)
3) the oxidation number of O is always -2, unless its just by itself (see #1)
4) the oxidation number of F is always -1, unless its just by itself (see#1)

ok so after you have written those oxidation numbers in rules 1-4 over each H, F, or O atom in the compound, you can look at the elements that we havent talked about yet

for example::::
N2O4

the oxidation number of O is -2.

since there are 4 O's, the charge is -8. now remember that N2O4 has to be neutral so the N2 must have a charge of +8
+8 divided by 2 = +4

N has an oxidation number of +4.

more rules:
5) the sum of oxidation numbers in a compound add up to 0 (when multiplied by the subscripts!!!) (see above example)
6) the sum of oxidation numbers in a polyatomic ion is the charge (for example, PO4 has a charge of (-3) so

oxidation # of O = -2. (there are 4 O's = -8 charge on that side ) P must have an oxidation number of 5. (-8+5= -3), and -3 is the total charge of the polyatomic ion

3 0

3 years ago

What is the mass of 2.90 ×1022 formula units of NaOH (Molar mass = 40.0 g/mol)?

enyata [817]

<h3>Solution:</h3>

$\text{mass of NaOH = 2.90 × 10²² NaOH formula units} × \frac{\text{1 mol NaOH}}{\text{6.022 × 10²³ NaOH formula units}} × \frac{\text{40.0 g NaOH}}{\text{1 mol NaOH}}$

$\boxed{\text{mass of NaOH = 1.926 g}}$

5 0

3 years ago

Read 2 more answers

5.75 moles of H2 gas to liters at STP

antiseptic1488 [7]

5.75mol (22.4L/1mol) = 128.8L

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3 years ago

Which phrase best describes how scientists use the data they collect

lozanna [386]

Answer:

The correct answer is b

7 0

3 years ago

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At 25C the density of water is 0.997044 g/mL. Use this value to determine the percent error for the two density measurements

Gnom [1K]

Given that:

At 25C the density of water is 0.997044 g/mL.

From the information attached below, we have the following parameters.

The density of water calculation using a bottle.

Initial volume of Final volume of Mass of water Density (g/mL)

burette (mL) burette (mL) dispensed (g)

Sample 1 2.33 7.34 5.000 -----

Sample 2 7.34 12.37 5.025 -----

Sample 3 12.37 18.50 6.112 -----

Sample 4 18.50 24.57 6.064 -----

Sample 5 24.57 31.31 6.720 -----

The first thing we need to do is to determine the change in the volume of the burette in each sample from the above information.

The change in the volume of the burette = (final volume - the initial volume) mL

Sample 1:

= (7.34 - 2.33) mL

= 5.01 mL

Sample 2:

= (12.37 - 7.34) mL

= 5.03 mL

Sample 3:

= (18.50 - 12.37) mL

= 6.03 mL

Sample 4:

= (24.57 - 18.50) mL

= 6.07 mL

Sample 5:

= (31.31 - 24.57) mL

= 6.74 mL

The mass of the water dispersed in sample 1 is given as = 5.000 g

Using the relation for calculating the density of each, we have:

Sample 1

$\mathbf{density = \dfrac{mass}{volume}}$

$\mathbf{density = \dfrac{5.01 g}{5.000 ml}}$

density = 0.998004 g/ml

Sample 2:

$\mathbf{density = \dfrac{5.025 g}{5.03ml}}$

density = 0.999006 g/ml

Sample 3:

$\mathbf{density = \dfrac{6.112 g}{6.13ml}}$

density = 0.997064 g/ml

Sample 4:

$\mathbf{density = \dfrac{6.064 \ g}{6.07 \ ml}}$

density = 0.999012 g/ml

Sample 5:

$\mathbf{density = \dfrac{6.720 \ g}{6.74 \ ml}}$

density = 0.997033 g/ml

Thus, the average density for all the samples is:

$\mathbf{= \dfrac{( 0.998004 + 0.999006 + 0.997064 + 0.999012 + 0.997033 )}{5}}$

= 0.998024

∴

The percentage error for the two densities measurement is:

$=\dfrac{ (experimental \ value -theoretical \ value)\times 100 }{theoretical \ value}$

Given that the theoretical value = 0.997044 g/ml

Then;

$\mathbf{= \dfrac{(0.998024 - 0.997044)100}{0.997044}}$

= 0.0983%

Therefore, we can conclude that the percent error for the two density measurements is 0.0983%

Learn more about density here:

brainly.com/question/24386693?referrer=searchResults

4 0

2 years ago