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Umnica [9.8K]
2 years ago
8

In the food web below, what is one example of an omnivore?

Chemistry
2 answers:
STALIN [3.7K]2 years ago
4 0
An omnivore is a animal that eats both meat, and plants.
I’m not too sure because most of these are omnivores so I think I would go for mouse or fox
Arada [10]2 years ago
3 0
Foxes are omnivores. so are mice.
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If 200. g of water at 20°C absorbs 41 840 J of energy, what will its final temperature be? (Specific Heat of water is 4.184 J/g*
Elena-2011 [213]

Answer: The final temperature will be 70^0C

Explanation:

To calculate the specific heat of substance during the reaction.

q=m\times c\times (T_{final}-T_{initial})

where,

q = heat absorbed =41840 J

c = specific heat = 4.184J/g^0C

m = mass of water  = 200 g

T_{final} = final temperature =?

T_{initial}= initial temperature = 20^0C

Now put all the given values in the above formula, we get:

41840J=200g\times 4.184J/g^0C\times (T_{final}-20)^0C

T_{final}=70^0C

Thus the final temperature will be 70^0C

3 0
3 years ago
A chemist determines by measurements that 0.030 moles of nitrogen gas participate in a chemical reaction. calculate the mass of
zzz [600]
Remember that: 
number of moles = mass/molar mass

First, we get the molar mass of the nitrogen gas molecule:
It is known the the nitrogen gas is composed of two nitrogen atoms, each with molar mass 14 gm (from the periodic table)
Therefore, molar mass of nitrogen gas = 14 x 2 = 28 gm

Second we calculate the mass of the precipitate:
we have number of moles = 0.03 moles (given)
and molar mass = 28 gm (calculated)
Using the equation mentioned before,
mass = number of moles x molar mass = 0.03 x 28 = 0.84 gm
3 0
3 years ago
CaBr + KOH – Ca(OH), + KBr (balance first) What mass, in grams, of
neonofarm [45]

Answer:

129.73 g of CaBr₂

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

CaBr₂ + 2KOH –> Ca(OH)₂ + 2KBr

Next, we shall determine the mass of CaBr₂ that reacted and the mass of Ca(OH)₂ produced from the balanced equation. This can be obtained as follow:

Molar mass of CaBr₂ = 40 + (80×2)

= 40 + 160

= 200 g/mol

Mass of CaBr₂ from the balanced equation = 1 × 200 = 200 g

Molar mass of Ca(OH)₂ = 40 + 2(16 + 1)

= 40 + 2(17)

= 40 + 34

= 74 g/mol

Mass of Ca(OH)₂ from the balanced equation = 1 × 74 = 74 g

SUMMARY :

From the balanced equation above,

200 g of CaBr₂ reacted to produce 74 g of Ca(OH)₂.

Finally, we shall determine the mass of CaBr₂ that react when 48 g of Ca(OH)₂ were produced. This can be obtained as follow:

From the balanced equation above,

200 g of CaBr₂ reacted to produce 74 g of Ca(OH)₂.

Therefore, Xg of CaBr₂ will react to produce 48 g of Ca(OH)₂ i.e

Xg of CaBr₂ = (200 × 48)/74

Xg of CaBr₂ = 129.73 g

Thus, 129.73 g of CaBr₂ were consumed.

6 0
3 years ago
How many inches are in 2.0 miles
erastovalidia [21]
126,720 inches are in 2.0 miles
3 0
3 years ago
How many mL will a 0.205 mole sample of He occupy at 3.00 atm and 200 K? Report your answer to the nearest mL.
Tcecarenko [31]

1.1214 mL will a 0.205-mole sample of He occupy at 3.00 atm and 200 K.

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

Using equation PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.

Given data:

P= 3.00 atm

V= ?

n=0.205 mole

R= 0.082057338 \;L \;atm \;K^{-1}mol^{-1}

T=200 K

Putting value in the given equation:

\frac{nRT}{P} =V

V= \frac{0.205 \;mole\;0.082057338 \;L \;atm \;K^{-1}mol^{-1} X 200}{3 \;atm}

V= 1.1214 mL

Learn more about the ideal gas here:

brainly.com/question/27691721

#SPJ1

4 0
2 years ago
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