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tester [92]
2 years ago
15

C6H12 + 9 O2 –> 6 CO2 + 6 H2O

Chemistry
1 answer:
baherus [9]2 years ago
6 0

5.76 g of O_2 are consumed when C_6H_1_2 is burned to yield 5.3 grams of CO_2.

<h3>What is a mole?</h3>

A mole is defined as 6.02214076 × 10^{23} of some chemical unit, be it atoms, molecules, ions, or others.

Calculating moles of CO_2

Number of mole of CO_2 = \frac{\;Given \;mass}{\;Molar \;mass}

\frac{\;Given \;mass}{\;Molar \;mass} = \frac{5.3g}{44 g/mol} = 0.12 mol

As is clear from the reaction stoichiometry, 9 moles of O_26 moles of CO_2.

Calculating the number of moles of CO_2

\frac{0.12 X 9}{6} = 0.18 mol

Mass of O_2 =5.76 g

Hence, 5.76 g of O_2 are consumed when C_6H_1_2 yield 5.3 grams of CO_2.

Learn more about mole here:

brainly.com/question/26416088

#SPJ1

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What is the relative atomic mass of a hypothetical element that consists isotopes in the indicated natural abundances
belka [17]

The given question is incomplete. The complete question is:What is the relative atomic mass of a hypothetical element that consists isotopes in the indicated natural abundances.

Isotope                    mass amu        Relative abundance

1                                77.9                     14.4

2                               81.9                     14.3

3                               85.9                      71.3

Express your answer to three significant figures and include the appropriate units.

Answer: 84.2 amu

Explanation:

Mass of isotope 1 = 77.9  

% abundance of isotope 1 = 14.4% = \frac{14.4}{100}=0.144

Mass of isotope 2 = 81.9

% abundance of isotope 2 = 14.3% = \frac{14.3}{100}=0.143

Mass of isotope 3 = 85.9

% abundance of isotope 2 = 71.3% = \frac{71.3}{100}=0.713

Formula used for average atomic mass of an element :

\text{ Average atomic mass of an element}=\sum(\text{atomic mass of an isotopes}\times {{\text { fractional abundance}})

A=\sum[(77.9\times 0.144)+(81.9\times 0.143)+(85.9\times 0.713)]

A=84.2amu

Therefore, the average atomic mass of a hypothetical element that consists isotopes in the indicated natural abundances is 84.2 amu

4 0
3 years ago
Given the following balanced chemical reaction:
Gnom [1K]

Answer:

Explanation:

according to balance chemical equation

  3 A2 moles produced 2 moles of A3B

so 12 moles A2 will produced moles of A3B= 12*2/3=24/3= 8

therefore 12 moles of A2 produced 8 moles of A3B

6 0
3 years ago
Which element has molecules containing 8 atoms?
motikmotik
I know that sulfur/sulphur does. It is commonly known as the sulfur s8 structure. 
6 0
3 years ago
The rate constant for the second-order reaction 2NOBr(g) ¡ 2NO(g) 1 Br2(g) is 0.80/M ? s at 108C. (a) Starting with a concentrat
Valentin [98]

Answer:

(a)

0.0342M

(b)

t_{1/2}=17.36s\\t_{1/2}=23.15s

Explanation:

Hello,

(a) In this case, as the reaction is second-ordered, one uses the following kinetic equation to compute the concentration of NOBr after 22 seconds:

\frac{1}{[NOBr]}=kt +\frac{1}{[NOBr]_0}\\\frac{1}{[NOBr]}=\frac{0.8}{M*s}*22s+\frac{1}{0.086M}=\frac{29.3}{M}\\

[NOBr]=\frac{1}{29.2/M}=0.0342M

(b) Now, for a second-order reaction, the half-life is computed as shown below:

t_{1/2}=\frac{1}{k[NOBr]_0}

Therefore, for the given initial concentrations one obtains:

t_{1/2}=\frac{1}{\frac{0.80}{M*s}*0.072M}=17.36s\\t_{1/2}=\frac{1}{\frac{0.80}{M*s}*0.054M}=23.15s

Best regards.

8 0
3 years ago
Read 2 more answers
HELP agaIN aSAPPPP!!!!!
Vinvika [58]

Answer:

D

the waves are actually being blocked

4 0
3 years ago
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