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Vesna [10]
3 years ago
7

1. An arch is a landform formed when wind picks up tiny bits of rock and sand and blows them against

Chemistry
1 answer:
Strike441 [17]3 years ago
8 0

Answer:

B

Explanation:

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PLEASE HELP<br><br> is this a chemical or physical change???
skad [1K]

Answer:

Chemical, cause physical are changes affecting the form of a chemical substance, but not its chemical composition. This doesn't affect the substance but the composition.

Explanation:

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3 years ago
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List the factor on which Ka of a weak acid depends​
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I don’t know this, so I did research, so here! This is from a website called “Quora”, btw!
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8 0
3 years ago
Objects that are able to fall have what type of energy?
ASHA 777 [7]

Answer:

kinetic energy

Explanation:

because of the movement of gravity and space

4 0
3 years ago
What is the excess reactant in the combustion of 23 g of methane in the open atmosphere?
Marta_Voda [28]

Answer : The excess reactant in the combustion of methane in opem atmosphere is O_{2} molecule.

Solution : Given,

Mass of methane = 23 g

Molar mass of methane = 16.04 g/mole

The Net balanced chemical reaction for combustion of methane is,

CH_4(g)+2O_2(g)\rightarrow CO_2(g)+2H_2O(g)

First we have to calculate the moles of methane.

\text{ Moles of methane}=\frac{\text{ Given mass of methane}}{\text{ Molar mass of methane}} = \frac{23g}{16.04g/mole} = 1.434 moles

From the above chemical reaction, we conclude that

1 mole of methane react with the 2 moles of oxygen

and 1.434 moles of methane react to give \frac{2moles\times 1.434moles}{1moles} moles of oxygen

The Moles of oxygen = 2.868 moles

Now we conclude that the moles of oxygen are more than the moles of methane.

Therefore, the excess reactant in the combustion of methane in open atmosphere is O_{2} molecule.


6 0
3 years ago
Chemistry Question, Don't really know how to do it lol.
Scilla [17]

Answer: 17.2 g

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}

\text{Moles of} HgS=\frac{20.0 g}{233g/mol}=0.085moles

The balanced chemical equation is:

4HgS(s)+4CaO(s)\rightarrow 4Hg(l)+3CaS(s))+CaSO_4(s)  

According to stoichiometry :  

4 moles of HgS produce =  4 moles of Hg

Thus 0.085 moles of HgS will require=\frac{4}{4}\times 0.085=0.085moles  of Hg

Mass of Hg=moles\times {\text {Molar mass}}=0.085moles\times 200.6g/mol=17.2g

Thus 17.2 g of Hg will be produced form 20.0 g of HgS.

3 0
2 years ago
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