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4 years ago

How many moles of copper are present in a sample of tennantite with a mass of 2290 grams?

Chemistry

1 answer:

grin007 [14]4 years ago

5 0

Answer:

18.58 moles of Cu

Solution:

Data Given:

Chemical Formula of Tennantite = Cu₁₂As₄S₁₃

Mass of Cu₁₂As₄S₁₃ = 2290 g

M.Mass of Cu₁₂As₄S₁₃ = 1479.06 g.mol⁻¹

Step 1: Calculate Moles of Cu₁₂As₄S₁₃ as,

Moles = Mass ÷ M.Mass

Putting values,

Moles = 2290 g ÷ 1479.06 g.mol⁻¹

Moles = 1.548 mol

Step 2: Calculate Moles of Cu,

As,

1 mole of Cu₁₂As₄S₁₃ contains = 12 moles of Cu

So,

1.548 mol of Cu₁₂As₄S₁₃ will contain = X moles of Cu

Solving for X,

X = (1.548 mol × 12 mol) ÷ 1 mol

X = 18.58 moles of Cu

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What makes organic compounds reactive?

konstantin123 [22]

Answer:

The functional groups

Explanation:

An organic compound is a compound that contain carbon and another element such as hydrogen, oxygen, nitrogen, etc.
Functional groups are the portions of an organic compound that is capable of characteristic reactions.
Functional groups determine the chemical and physical properties of many organic compounds.

3 0

4 years ago

1. How many joules must be added to 10.0 g of water to raise its temperature from 10°C to<br> 15°C?

weqwewe [10]

Answer:

209.3 Joules require to raise the temperature from 10 °C to 15 °C.

Explanation:

Specific heat capacity:

It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Formula:

Q = m × c × ΔT

Given data:

mass of water = 10 g

initial temperature T1= 10 °C

final temperature T2= 15 °C

temperature change =ΔT= T2-T1 = 15°C - 10°C = 5 °C

Energy or joules added to increase the temperature Q = ?

Solution:

We know that specific heat of water is 4.186 J/g .°C

Q = m × c × ΔT

Q = 10 g × 4.186 J/g .°C × 5 °C

Q = 209.3 J

6 0

3 years ago

Consider the incomplete structure. Add formal charges as necessary to the structure. All unshared valence electrons are shown.

Zina [86]

The net charge on the structure as shown in the question is -1.

<h3>What is a charged specie?</h3>

We say that a specie is charged if the specie has an excess of positive or negative charge. An excess of the positive charge means that the substance is positively charged while an excess if the negative charge simply means that the object is negative charged.

When we have a chemical structure as we have seen, it is possible that the structure as we have it could have a net charge. The net charge that the structure has can be deduced by looking at the formal charges that are carried by all the atoms that we have in the system.

The charge as we can see that is on the central atom of the molecule is the -1 charge hence this is the charge that is carried overall by the molecule.

If we then look at the structure as we can see, we can see that there is a charge of negative one that is attached to the atom of chlorine as is clearly visible and obvious from the image attached to the question.

Learn more about net charge:brainly.com/question/12708636

#SPJ1

5 0

1 year ago

How many grams of O2 are present in 44.1 L of O2 at STP?

ycow [4]

Taking into accoun the STP conditions and the ideal gas law, the correct answer is option e. 63 grams of O₂ are present in 44.1 L of O2 at STP.

First of all, the STP conditions refer to the standard temperature and pressure, where the values used are: pressure at 1 atmosphere and temperature at 0°C. These values are reference values for gases.

On the other side, the pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P×V = n×R×T

where:

P is the gas pressure.
V is the volume that occupies.
T is its temperature.
R is the ideal gas constant. The universal constant of ideal gases R has the same value for all gaseous substances.
n is the number of moles of the gas.

Then, in this case:

P= 1 atm
V= 44.1 L
n= ?
R= 0.082 $\frac{atmL}{molK}$
T= 0°C =273 K

Replacing in the expression for the ideal gas law:

1 atm× 44.1 L= n× 0.082 $\frac{atmL}{molK}$ × 273 K

Solving:

$n=\frac{1 atm x44.1 L}{0.082\frac{atmL}{molK}x273K}$

n=1.97 moles

Being the molar mass of O₂, that is, the mass of one mole of the compound, 32 g/mole, the amount of mass that 1.97 moles contains can be calculated as:

$1.97 molesx\frac{32 g}{1 mole}$ = 63.04 g ≈ <u><em>63 g</em></u>

Finally, the correct answer is option e. 63 grams of O₂ are present in 44.1 L of O2 at STP.

Learn more about the ideal gas law:

<u>brainly.com/question/4147359?referrer=searchResults</u>

7 0

3 years ago

If 832J of energy is required to raise the temperature of a sample of aluminum from 20.0° C to 97.0° C, what mass is the sample

LiRa [457]

Data:
Q (Amount of heat) = 832 J
m (mass) = ?
c (Specific heat) = <span>0.90 J/(g × ° C)
T (final) = 97 ºC
To (initial) = 20 ºC
</span>ΔT = T - To → ΔT = 97 - 20 → ΔT = 77 ºC

Formula:
Q = m*c*ΔT

Solving:
Q = m*c*ΔT
832 = m*0.90*77
832 = 69.3m
69.3m = 832
$m = \frac{832}{69.3}$
$\boxed{\boxed{m \approx 12.00\:g}}\end{array}}\qquad\quad\checkmark$

5 0

3 years ago