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3 years ago

13

Let me know the answer to this oneeee

1 answer:

defon3 years ago

8 0

<h2><em>Answer:</em></h2>

<em>1</em><em>.</em><em>2</em><em> </em><em>moles </em><em>of </em><em>hydrogen</em>

<em>please </em><em>see</em><em> the</em><em> attached</em><em> picture</em>

<em>hope </em><em>it</em><em> helps</em>

<em>Good </em><em>luck</em><em> on</em><em> your</em><em> assignment</em>

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An experiment requires 50.0 mL of 0.040 M NaOH for the titration of 1.00 mmol of acid. Mass analysis of the acid shows 2.24% hyd

tino4ka555 [31]

The molecular formula is calculated as follows

that is for carbon = 26.7/12= 2.23 moles

hydrogen= 2.24/1=2.24 moles

oxygen= 71.1/16=4.44 moles

<h3> What is molecular formula?</h3>

A chemical formula is a way to describe the chemical ratios of the atoms that make up a specific chemical compound or molecule in chemistry. Chemical element symbols, numbers, and occasionally other symbols, such as parentheses, dashes, brackets, commas, and plus (+) and minus () signs, are used to represent the chemical elements. These can only include one typographic line of symbols, which may also include subscripts and superscripts. A chemical formula has no words and is not the same as the chemical name. A chemical formula does not equal a complete chemical structural formula, despite the fact that it may suggest some basic chemical structures. Chemical formulae are often less powerful than chemical names and structural formulae, and they can only fully describe the structure of the simplest molecules and chemical compounds.

To learn more about molecular formula from the given link:

brainly.com/question/14425592

#SPJ4

8 0

2 years ago

1. Related to the number of particles in a gram of

Romashka-Z-Leto [24]

Answer:

Avogadro's number or Avogardro’s constant

Explanation:

I’m pretty sure this is correct if it’s not I’m sorry lol.

6 0

2 years ago

A student has a 2.19 L bottle that contains a mixture of O 2 , N 2 , and CO 2 with a total pressure of 5.57 bar at 298 K . She k

Sergeeva-Olga [200]

<u>Answer:</u> The partial pressure of oxygen gas is 2.76 bar

<u>Explanation:</u>

To calculate the number of moles, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = 5.57 bar

V = Volume of the gas = 2.19 L

T = Temperature of the gas = 298 K

R = Gas constant = $0.0831\text{ L bar }mol^{-1}K^{-1}$

n = Total number of moles = ?

Putting values in above equation, we get:

$5.57bar\times 2.19L=n\times 0.0831\text{ L. bar }mol^{-1}K^{-1}\times 298K\\\\n=\frac{5.57\times 2.19}{0.0831\times 298}=0.493mol$

To calculate the mole fraction of carbon dioxide, we use the equation given by Raoult's law, which is:

$p_{A}=p_T\times \chi_{A}$ ........(1)

where,

$p_A$ = partial pressure of carbon dioxide = 0.318 bar

$p_T$ = total pressure = 5.57 bar

$\chi_A$ = mole fraction of carbon dioxide = ?

Putting values in above equation, we get:

$0.318bar=5.57bar\times \chi_{CO_2}\\\\\chi_{CO_2}=\frac{0.381}{5.57}=0.0571$

Mole fraction of a substance is given by:

$\chi_A=\frac{n_A}{n_A+n_B}$

We are given:

Moles of nitrogen gas = 0.221 moles

Mole fraction of nitrogen gas, $\chi_{N_2}=\frac{0.221}{0.493}=0.448$

Calculating the partial pressure of oxygen gas by using equation 1, we get:

Mole fraction of oxygen gas = (1 - 0.0571 - 0.448) = 0.4949

Total pressure of the system = 5.57 bar

Putting values in equation 1, we get:

$p_{O_2}=5.57bar\times 0.4949\\\\p_{O_2}=2.76bar$

Hence, the partial pressure of oxygen gas is 2.76 bar

6 0

4 years ago

Ocean basins will expand as new oceanic crust forms and moves away from a mid-oceanic ridge during

KATRIN_1 [288]

Sea floor spread ing

4 0

3 years ago

Read 2 more answers

What is the correct chemical equation for the reaction between methane and oxygen to produce carbon dioxide and water?

kodGreya [7K]

Answer:

The answer to your question is: CH₄ + 3/2 O₂ ⇒ CO₂ + 2 H₂O

Explanation:

Methane = CH₄

Oxygen = O

Carbon dioxide = CO₂

Water = H₂O

CH₄ + 3/2 O₂ ⇒ CO₂ + 2 H₂O

This is the balanced equation

3 0

3 years ago