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Olin [163]
3 years ago
14

Combustion of hydrogen releases 142 j/g of hydrogen reacted. How many kj of energy are released by the combustion of 16.0 oz of

hydrogen? (1 lb = 16 oz; 1 kg = 2.2 lb)

Chemistry
2 answers:
Delvig [45]3 years ago
7 0

64.61 kJ of energy is released by the combustion of 16.0 oz of hydrogen

<h3>Further explanation</h3>

Delta H reaction (ΔH) is the amount of heat/heat change between the system and its environment

(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)

The reaction of a substance with oxygen is called a combustion reaction

the combustion of hydrogen is

<h3>2H₂ + O₂ → 2H₂O.</h3>

This equation shows that 2 Hydrogen molecules react with 1 molecule of oxygen to produce 2 molecules of water

In this combustion reaction will produce large thermal energy because it involves breaking the hydrogen gas bond, so the reaction is exothermic

The combustion of hydrogen releases 142 j / g of hydrogen reacted.

Combustion of 16.0 oz of hydrogen will release heat of:

16 oz = 1 lb = 0.455 kg = 455 g

For each gram Hydrogen releases 142 J, then for 455 g releases:

142 x 455 J = 64610 J = 64.61 kJ

<h3>Learn more</h3>

the complete combustion of methane

brainly.com/question/1971314

grams of o2 are required to burn 17.0 gal of c8h18

brainly.com/question/5816411#

moles of oxygen are required to produce 2.33 moles of water

brainly.com/question/6209439

Keywords: Combustion of hydrogen, ΔH reaction, water, oxygen, exothermic

Andrej [43]3 years ago
5 0

Given the mass of hydrogen = 16.0 oz

Converting 16.0 oz hydrogen to pounds (lb) using the conversion factor 1 lb = 16 oz:

16.0 oz * \frac{1 lb}{16 oz} =1 lb

Converting 16.0 lb to g using the conversion factors 1 kg = 2.2 lb, 1 kg = 1000 g:

1lb * \frac{1kg}{2.2lb}*\frac{1000g}{1kg}= 454.5 g

Heat of combustion of hydrogen = 142 J/g

Calculating the heat released when 16.0 oz is combusted:

454.5g H_{2} * \frac{142 J}{g} *\frac{1 kJ}{1000J}=64.5kJ


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Starting with the stock solution of 6.0 M, how many milliliters of 6.0 M sulfuric acid are needed to make 450 mL of 1.2 M soluti
Lina20 [59]

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<u>Explanation:</u>

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6 0
3 years ago
Can anyone help me on this please?
Bad White [126]
This question is testing to see how well you understand the "half-life" of radioactive elements, and how well you can manipulate and dance around them.  This is not an easy question.

The idea is that the "half-life" is a certain amount of time.  It's the time it takes for 'half' of the atoms in any sample of that particular unstable element to 'decay' ... their nuclei die, fall apart, and turn into nuclei of other elements.

Look over the table.  There are 4,500 atoms of this radioactive substance when the time is 12,000 seconds, and there are 2,250 atoms of it left when the time is ' y ' seconds.  Gosh ... 2,250 is exactly half of 4,500 !  So the length of time from 12,000 seconds until ' y ' is the half life of this substance !  But how can we find the length of the half-life ? ? ?

Maybe we can figure it out from other information in the table !

Here's what I found:

Do you see the time when there were 3,600 atoms of it ? 
That's 20,000 seconds.

... After one half-life, there were 1,800 atoms left.
... After another half-life, there were 900 atoms left.
... After another half-life, there were 450 atoms left. 

==>  450 is in the table !  That's at 95,000 seconds.

So the length of time from 20,000 seconds until 95,000 seconds
is three half-lifes.

The length of time is (95,000 - 20,000) = 75,000 sec

                                     3 half lifes = 75,000 sec

Divide each side by 3 :   1 half life = 25,000 seconds

There it is !  THAT's the number we need.  We can answer the question now.

==> 2,250 atoms is half of 4,500 atoms.

==> ' y ' is one half-life later than 12,000 seconds

==> ' y ' = 12,000 + 25,000

         y   = 37,000 seconds  .

Check: 
Look how nicely 37,000sec fits in between 20,000 and 60,000 in the table.

As I said earlier, this is not the simplest half-life problem I've seen.
You really have to know what you're doing on this one.  You can't
bluff through it.


7 0
3 years ago
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