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3 years ago

What are the lessons that you learn from nature

Chemistry

2 answers:

Daniel [21]3 years ago

7 0

Answer:

Nature is important

Explanation:

Nesterboy [21]3 years ago

3 0

To appreciate small things,
like how flowers appreciate it when bees pollinate them, or how animals appreciate it when people feed them

You might be interested in

What is responsible for changes in the state of matter?

NeX [460]

Answer:

Temperature and pressure are the two factors which are responsible for change in state of matter.

Solid – In a solid, the attractive forces keep the particles together tightly enough so that the particles do not move past each other. ... In the solid the particles vibrate in place. Liquid – In a liquid, particles will flow or glide over one another, but stay toward the bottom of the container.

<em>Hope this helps, mark as Brainliest please...</em>

8 0

3 years ago

20 POINTS Use the problem below to answer the question: 34 grams of carbon react with an unlimited amount of H2O. The reaction i

Simora [160]

The carbon would be your answer hope this helps

4 0

3 years ago

What is one source of organic matter in soil ?

stealth61 [152]

The original source of the soil organic matter is plant tissue. In the forest, organic matter is added in the soil mainly in the form of fallen leaves. Under natural conditions, the tops and roots of trees, shrubs, grasses and other native plants annually supply large quantities of organic residues.

3 0

3 years ago

8. A sample of potassium chlorate (KCIO,) was heated in a test tube and decomposed 2KC?(s) 302 (g) + 2KCIO, (s) The oxygen was c

dangina [55]

Answer:

Partial pressure of $O_{2}$ in the gas was 733 torr and mass of $KClO_{3}$ in the sample was 2.12 g.

Explanation:

a) Total pressure of gas = (partial pressure of water vapour)+(partial pressure of $O_{2}$ )

Here partial pressure of water vapour is 21 torr and total pressure of gas is 754 torr.

So, partial pressure of $O_{2}$ = (total pressure of gas)-(partial pressure of water vapour) = (754 torr) - (21 torr) = 733 torr

b) Lets assume that $O_{2}$ behaves ideally. Hence-

PV=nRT

where P is pressure of $O_{2}$ , V is volume of $O_{2}$ , n is number of moles of $O_{2}$ , R is gas constant and T is temperature in kelvin

here P = 733 torr = $(733\times 0.001316)atm$ = 0.9646 atm

V = 0.65 L, R = 0.082 L.atm/(mol.K), T=(273+22)K = 295 K

So, $n=\frac{PV}{RT}$

= $\frac{(0.9646 atm)\times (0.65 L)}{(0.082 L.atm/(mol.K))\times (295 K)}$

= 0.0259 moles

As 3 moles of $O_{2}$ are produced from 2 moles of $KClO_{3}$ therefore 0.0259 moles of $O_{2}$ are produced from $(\frac{2\times 0.0259}{3})$ moles or 0.0173 moles of $KClO_{3}$ .

Molar mass of $KClO_{3}$ = 122.55 g

So mass of $KClO_{3}$ in sample = $(0.0173\times 122.55)g$

= 2.12 g

7 0

3 years ago

How many grams of K2O will be produced from 0.50 g of K<br> and 0.10 g of O2?

Rudik [331]

Answer:

0.6g

Explanation:

Given parameters:

Mass of K = 0.5g

Mass of O₂ = 0.10g

Unknown:

Mass of K₂O = ?

Solution:

To solve this problem, let us write the reaction equation first;

4K + O₂ → 2K₂O

The reaction above delineates the balanced chemical reaction.

To solve this problem, we need to know the limiting reactant. This reactant is the one that determines the amount and extent of the reaction because it is given in short supply. The other reactant is the one in excess.

Start off by find the number of moles of the reactant;

Number of moles = $\frac{mass}{molar mass}$