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3 years ago

How to learn chemistry?

Chemistry

1 answer:

melamori03 [73]3 years ago

8 0

Answer:

Chemistry Study Guide

How To Study for Chemistry

Chemistry is one of those classes you either love or dread. At the high school level chemistry is usually not a required course – it's an elective. However, most reputable colleges require all undergraduate students to take at least one chemistry course as a prerequisite to graduation. If you plan on pursuing a career in medicine, engineering, or a field of natural science, then you're likely going to be required to take at least one chemistry course before you graduate. Chemistry is a challenging subject for most people, but it doesn't have to be. The number one reason people struggle with chemistry is that they don't approach it the right way. Below we'll explore proven strategies and techniques that will, if applied, improve your ability to study and learn chemistry.

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Which greenhouse gas is emitted when people burn fossil fuels for energy?

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It would be carbon dioxide because carbon dioxide makes up the vast majority of greenhouse gas .

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3 years ago

What is a characteristic of asexual reproduction?

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Answer:

Sexual reproduction

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3 years ago

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The following is what type of reaction: 2Al(s) + 3CuCl2(aq) ---> 2AlCl3(aq) + 3Cu(s)

Volgvan

Answer:

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3 years ago

Find the enthalpy of neutralization of HCl and NaOH. 137 cm3 of 2.6 mol dm-3 hydrochloric acid was neutralized by 137 cm3 of 2.6

liraira [26]

Answer : The correct option is, (D) 89.39 KJ/mole

Explanation :

First we have to calculate the moles of HCl and NaOH.

$\text{Moles of HCl}=\text{Concentration of HCl}\times \text{Volume of solution}=2.6mole/L\times 0.137L=0.3562mole$

$\text{Moles of NaOH}=\text{Concentration of NaOH}\times \text{Volume of solution}=2.6mole/L\times 0.137L=0.3562mole$

The balanced chemical reaction will be,

$HCl+NaOH\rightarrow NaCl+H_2O$

From the balanced reaction we conclude that,

As, 1 mole of HCl neutralizes by 1 mole of NaOH

So, 0.3562 mole of HCl neutralizes by 0.3562 mole of NaOH

Thus, the number of neutralized moles = 0.3562 mole

Now we have to calculate the mass of water.

As we know that the density of water is 1 g/ml. So, the mass of water will be:

The volume of water = $137ml+137ml=274ml$

$\text{Mass of water}=\text{Density of water}\times \text{Volume of water}=1g/ml\times 274ml=274g$

Now we have to calculate the heat absorbed during the reaction.

$q=m\times c\times (T_{final}-T_{initial})$

where,

q = heat absorbed = ?

$c$ = specific heat of water = $4.18J/g^oC$

m = mass of water = 274 g

$T_{final}$ = final temperature of water = 325.8 K

$T_{initial}$ = initial temperature of metal = 298 K

Now put all the given values in the above formula, we get:

$q=274g\times 4.18J/g^oC\times (325.8-298)K$

$q=31839.896J=31.84KJ$

Thus, the heat released during the neutralization = -31.84 KJ

Now we have to calculate the enthalpy of neutralization.

$\Delta H=\frac{q}{n}$

where,

$\Delta H$ = enthalpy of neutralization = ?

q = heat released = -31.84 KJ

n = number of moles used in neutralization = 0.3562 mole

$\Delta H=\frac{-31.84KJ}{0.3562mole}=-89.39KJ/mole$

The negative sign indicate the heat released during the reaction.

Therefore, the enthalpy of neutralization is, 89.39 KJ/mole

3 0

4 years ago

If 5.100 g of c6h6 is burned and the heat produced from the burning is added to 5691 g of water at 21 °c, what is the final temp

emmasim [6.3K]

<span>C6H12 = 6x12 + 6x1 = 78.
The equation indicates that 2x78 = 156g benzene will produce 6542kJ.
Using proportions you can then calculate that
x/6542kJ = 7.9g / 156g
x = 331.3kJ = 331300J.

heat = mass x ΔT x 4.18J/g°
ΔT = 331300J / (5691g x 4.18J/g°) = 13.9°

final temp = 21 + 14° = 35°C</span>

4 0

3 years ago

How to learn chemistry?​

How to learn chemistry?