8. The threats to biodiversity are except:.

What happens to most of the Energy that an organism gets from consuming food? <br><br>Help please

kobusy [5.1K]

It’s the second answer. “it gets used for metabolic process & released as heat” i think.

7 0

2 years ago

The temperature of a 500. ml sample of gas increases from 150. k to 350. k. what is the final volume of the sample of gas, if th

maw [93]

<span>pv=nrt; Pressure and moles are constant. p=nr(150k)/.5 L; Pressure initially After temp change pv=nrt; What is volume? v=nr(350k)/p; p is constant so we can substitute from above v=nr(350k)/(nr(150k)/.5 L)) v=350/150/.5 L v=4.66 liters</span>

3 0

3 years ago

Read 2 more answers

Which statement describes the bonds in iron sulfate, FeSO4?

Feliz [49]

___

Regarding the bonds in FesO₄, Fe and S have an ionic bond, while S and O have covalent bonds.

Elements form bonds to increase their stability. The main types of bonds are:

Metallic bonds: they are formed between metals and the electrons are in a delocalized cloud.
Ionic bonds: they are formed between metals (lose electrons) and nonmetals (gain electrons)
Covalent bonds: they are formed between nonmetals, which share electrons.

Regarding the bonds in FesO₄:

Fe is a metal and S a nonmetal, thus they will form ionic bonds.
S and O are both nonmetals, thus they will form covalent bonds.

Regarding the bonds in FesO₄, Fe and S have an ionic bond, while S and O have covalent bonds.

Learn more: brainly.com/question/23882847

5 0

2 years ago

A chemist encounters an unknown metal. They drop the metal into a graduated cylinder containing water, and find the volume chang

Mashutka [201]

Answer:

The density of the metal is 0.561 g/mL

Explanation:

The computation of the density of the metal is shown below;

As we know that

The Density of the metal is

$= \frac{mass}{volume}$

where,

Mass = 4.9g

Change in volume = 6.9 mL

Now place these values to the above formula

So, the density of the metal is

$= \frac{4.9g}{6.9mL}$

= 0.561 g/mL

Hence, the density of the metal is 0.561 g/mL

We simply applied the above formula so that the correct density could arrive

5 0

3 years ago

Using the thermodynamic information in the ALEKS Data tab, calculate the boiling point of titanium tetrachloride . Round your an

ddd [48]

Answer:

The boiling point is 308.27 K (35.27°C)

Explanation:

The chemical reaction for the boiling of titanium tetrachloride is shown below:

Ti $Cl_{4(l)}$ ⇒ Ti $Cl_{4(g)}$

ΔH° $_{f}$ (Ti $Cl_{4(l)}$ ) = -804.2 kJ/mol

ΔH° $_{f}$ (Ti $Cl_{4(g)}$ ) = -763.2 kJ/mol

Therefore,

ΔH° $_{f}$ = ΔH° $_{f}$ (Ti $Cl_{4(g)}$ ) - ΔH° $_{f}$ (Ti $Cl_{4(l)}$ ) = -763.2 - (-804.2) = 41 kJ/mol = 41000 J/mol

Similarly,

s°(Ti $Cl_{4(l)}$ ) = 221.9 J/(mol*K)

s°(Ti $Cl_{4(g)}$ ) = 354.9 J/(mol*K)

Therefore,

s° = s° (Ti $Cl_{4(g)}$ ) - s°(Ti $Cl_{4(l)}$ ) = 354.9 - 221.9 = 133 J/(mol*K)

Thus, T = ΔH° $_{f}$ /s° = [41000 J/mol]/[133 J/(mol*K)] = 308. 27 K or 35.27°C

Therefore, the boiling point of titanium tetrachloride is 308.27 K or 35.27°C.

5 0

3 years ago