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3 years ago

If hydrogen and oxygen were to chemically bond together, what kind of bond would be created

1 answer:

5 0

Water dude lol H²0 (dont you know?) #rhymes

H²o → Hydrogen [The 2 means there are two hydrogen atoms], Oxygen = H²O

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Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decoxide and water, as

erica [24]

<u>Answer:</u> The amount of $P_4O_{10}$ formed is 469.8 grams.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ......(1)

Given mass of phosphine = 225 g

Molar mass of phosphine = 34 g/mol

Putting values in equation 1, we get:

$\text{Moles of phosphine}=\frac{225g}{34g/mol}=6.62mol$

The given chemical reaction follows:

$4PH_3(g)+8O_2(g)\rightarrow P_4O_{10}(s)+6H_2O(g)$

Assuming that oxygen gas is present in excess, it is considered as an excess reagent.

Phosphine is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

4 moles of phosphine produces 1 mole of $P_4O_{10}$

So, 6.62 moles of phosphine will produce = $\frac{1}{4}\times 6.62=1.655mol$ of $P_4O_{10}$

Now, calculating the mass of $P_4O_{10}$ by using equation 1:

Molar mass of $P_4O_{10}$ = 283.9 g/mol

Moles of $P_4O_{10}$ = 1.655 moles

Putting values in equation 1, we get:

$1.655mol=\frac{\text{Mass of }P_4O_{10}}{283.9g/mol}\\\\\text{Mass of }P_4O_{10}=(1.655mol\times 283.9g/mol)=469.8g$

Hence, the amount of $P_4O_{10}$ formed is 469.8 grams.

8 0

3 years ago

What is the significance of a gene?Immersive Reader

Ilia_Sergeevich [38]

Explanation:

A gene is the basic physical and functional unit of heredity. Genes are made up of DNA. Every person has two copies of each gene, one inherited from each parent. Most genes are the same in all people, but a small number of genes (less than 1 percent of the total) are slightly different between people. These small differences contribute to each person’s unique physical features.

4 0

3 years ago

Curious Carl conducted an experiment on the eating habits of black bears. While living in the woods, Carl was able to record the

Gnom [1K]

Answer:

Explanation:

I just got it correct.

6 0

3 years ago

Read 2 more answers

Why is pure silicon a poor conductor at room temperature

Serga [27]

It has 4 valence electron, all of which are needed to bond with nearest neighbors

6 0

3 years ago

What is the number of moles in 500 L of He gas at STP

earnstyle [38]

Answer:

20 moles

Explanation:

The important thing to realize here is that you're working under STP conditions, which implies that you can use the molar volume of a gas at STP to find how many moles of helium will occupy that volume.
Now, the molar volume of a gas represents the volume occupied by one mole of a gas under some specific conditions for pressure and temperature.
Starting from the ideal gas law equation

PV=nRT

you can say that the molar volume of gas at a pressure P and a temperature T will be equal to

Vn=RTP

Now, Standard Temperature and Pressureconditions are defined as a pressure of 100 kPaand a temperature of 0∘C. Under these specific conditions, the molar volume of a gas will be equal to

Vn=0.0821⋅atm⋅Lmol⋅K⋅(273.15+0)K100101.325atm
Vn=22.7 L/mol

This of course implies that one mole of any ideal gas will occupy 22.7 L.
In your case, the volume of the gas is said to be equal to 500 L. This means that you will have

500L⋅1 mole He22.7L=22.026 moles He

Rounded to one sig fig, the number of sig figs you have for the volume of the gas, the answer will be

nHe=20 moles

SIDE NOTE Many textbooks and online sources still list STP conditions as a pressure of 1 atmand a temperature of 0∘C.
Under these conditions for pressure and temperature, one mole of any ideal gas occupies 22.4 L. If these are the values for STP given to you by your instructor, make sure to redo the calculations using 22.4 L instead of 22.7 L

6 0

3 years ago

Read 2 more answers