SUSTANTIVO FORMA TAMANO CO

2c+02=2CO2. The moles of co2 produced when 0.25 moles of O2 react is?

Sophie [7]

<h3>Answer:</h3>

$\displaystyle 0.5 \ mol \ CO_2$

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right<u> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

Moles
Compounds

<u>Stoichiometry</u>

Using Dimensional Analysis
Analyzing Reactions RxN

<h3>Explanation:</h3>

<u>Step 1: Define</u>

[RxN - Balanced] 2C + O₂ → 2CO₂

[Given] 0.25 moles O₂

[Solve] moles CO₂

<u>Step 2: Identify Conversions</u>

[RxN] 1 mol O₂ → 2 mol CO₂

<u>Step 3: Stoichiometry</u>

[DA] Set up: $\displaystyle 0.25 \ moles \ O_2(\frac{2 \ mol \ CO_2}{1 \ mol \ O_2})$
[DA] Multiply/Divide [Cancel out units]: $\displaystyle 0.5 \ mol \ CO_2$

7 0

2 years ago

Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO) and gaseous water (H2O) . Suppo

Leto [7]

Answer:

0 g.

Explanation:

Hello,

In this case, since the reaction between methane and oxygen is:

$CH_4+2O_2\rightarrow CO_2+2H_2O$

If 0.963 g of methane react with 7.5 g of oxygen the first step is to identify the limiting reactant for which we compute the available moles of methane and the moles of methane consumed by the 7.5 g of oxygen:

$n_{CH_4}=0.963gCH_4*\frac{1molCH_4}{16gCH_4}=0.0602molCH_4\\ \\n_{CH_4}^{consumed}=7.5gO_2*\frac{1molO_2}{32gO_2}*\frac{1molCH_4}{2molO_2} =0.117molCH_4$

Thus, since oxygen theoretically consumes more methane than the available, we conclude the methane is the limiting reactant, for which it will be completely consumed, therefore, no remaining methane will be left over.

$left\ over=0g$

Regards.

7 0

3 years ago

Which element was first discovered in space before it was discovered on Earth?

faltersainse [42]

Helium was first discovered in space before it was on earth

7 0

3 years ago

Read 2 more answers

Nickel (II) oxide reacts with carbon monoxide to form nickel metal. CO(g) + NiO(s) ⇄ CO2(g) + Ni(s) Kp = 20 at 873 K If a reacti

ozzi

Answer:

Explanation:

Hello,

Based on the statement of the equilibrium law:

$Kp=\frac{P_{CO_2}^{EQ}}{P_{CO}^{EQ}}$

By increasing (doubling) the amount of carbon monoxide, the production of nickel will increase since its amount is directly proportional with its pressure, so, by adding more reactant (in this case carbon monoxide), the equilibrium is rightward shifted based on Le Châtelier's principle even when solid either reactants or products are not contemplated in the equilibrium law.

Best regards.

4 0

3 years ago

How many moles of BCl3 are needed to produce 10.0 g of HCl(aq) in the following reaction? (HCl molar mass is 36.46 g/mol).

Scilla [17]

Answer:

Moles of BCl₃ needed = 0.089 mol

Explanation:

Given data:

Moles of BCl₃ needed = ?

Mass of HCl produced = 10.0 g

Solution:

Chemical equation:

BCl₃ + 3H₂O → 3HCl + B(OH)₃

Number of moles of HCl:

Number of moles = mass/molar mass

Number of moles = 10.0 g/ 36.46 g/mol

Number of moles = 0.27 mol

Now we will compare the moles of HCl with BCl₃.

HCl : BCl₃

3 : 1

0.27 : 1/3×0.27 = 0.089 mol

6 0

2 years ago