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3 years ago

9

a bird population only eats a certain type of plant. one year, flooding washes away most of these plants in an area. what will m

ost likely result?

2 answers:

icang [17]3 years ago

8 0

Answer:

emigration followed by competition?

Explanation:

uh, yea?

kvv77 [185]3 years ago

6 0

A reduction of the bird population in that particular area.

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A textbook measures 250 mm long, 225 mm wide and 50 mm thick. What is the volume of this book in mm3? What is the volume of this

Dvinal [7]

Answer:

2.81 × 10⁶ mm³

2.81 × 10⁻³ m³

Explanation:

Step 1: Given data

Length (l): 250 mm

Width (w): 225 mm

Thickness (t): 50 mm

Step 2: Calculate the volume of the textbook

The book is a cuboid so we can find its volume (V) using the following expression.

V = l × w × t = 250 mm × 225 mm × 50 mm = 2.81 × 10⁶ mm³

Step 3: Convert the volume to cubic meters

We will use the relationship 1 m³ = 10⁹ mm³.

2.81 × 10⁶ mm³ × 1 m³ / 10⁹ mm³ = 2.81 × 10⁻³ m³

6 0

3 years ago

What the different betwen observe and reference

NNADVOKAT [17]

Observe to to gather facts, by paying close attention towards what you are working on.

meanwhile, reference is the act or process on reaching to your conclusion, based on facts you already know .

7 0

3 years ago

A 1.25 g gas sample occupies 663 ml at 25∘ c and 1.00 atm. what is the molar mass of the gas?

lakkis [162]

Using ideal gas equation,

$P\times V=n\times R\times T$

Here,

P denotes pressure

V denotes volume

n denotes number of moles of gas

R denotes gas constant

T denotes temperature

The values at STP will be:

P=1 atm

T=25 C+273 K =298.15K

V=663 ml=0.663L

R=0.0821 atm L mol ⁻¹

Mass of gas given=1.25 g g

Molar mass of gas given=?

$Number of moles of gas, n= \frac{Given mass of the gas}{Molar mass of the gas}$

$Number of moles of gas, n= \frac{1.25}{Molar mass of the gas}$

Putting all the values in the above equation,

$1\times 0.663=\frac{1.25}{Molar mass of the gas}\times 0.0821\times 298.15$

Molar mass of the gas=46.15

3 0

3 years ago

Chlorine is the most widely used disinfectant for killing pathogens during water treatment. Determine the kilograms of chlorine

makkiz [27]

Explanation:

The given data is as follows.

Flow of chlorine (Q) = $10,000 m^{3}/day$

Amount of liter present per day is as follows.

$10,000 \times 10^{3} l/day$

It is given that dosage of chlorine will be as follows.

10 mg/l = $10 \times 10^{-6}$ kg/l

Therefore, total chlorine requirement is as follows.

Total chlorine requirement = $(10,000 \times 10^{3}) \times (10 \times 10^{-6})$ kg/day

= 100 kg/day

Thus, we can conclude that the kilograms of chlorine used daily at the given water treatment plant is 100 kg/day.

4 0

3 years ago

13. What is the total pressure inside the container

nasty-shy [4]

<u>Answer:</u> The total pressure inside the container is 77.9 kPa

<u>Explanation:</u>

Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.

To calculate the total pressure inside the container, we use the law given by Dalton, which is:

$P_T=p_{N_2}+p_{O_2}+p_{Ar}$

We are given:

Vapor pressure of oxygen gas, $p_{O_2}$ = 40.9 kPa

Vapor pressure of nitrogen gas, $p_{N_2}$ = 23.3 kPa

Vapor pressure of argon, $p_{Ar}$ = 13.7 kPa

Putting values in above equation, we get:

$p_T=23.3+40.9+13.7\\\\p_{T}=77.9kPa$

Hence, the total pressure inside the container is 77.9 kPa

7 0

3 years ago