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lana66690 [7]
3 years ago
14

You have 15.42g of C2H6. How many moles of H2O can be made?

Chemistry
1 answer:
Amiraneli [1.4K]3 years ago
4 0

<u>Answer:</u> The moles of water produced are 1.54 moles.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass of ethane = 15.42 g

Molar mass of ethane = 30.07 g/mol

Putting values in above equation, we get:

\text{Moles of ethane}=\frac{15.42g}{30.07g/mol}=0.513mol

The chemical equation for the combustion of ethane follows:

2C_2H_6+5O_2\rightarrow 4CO2+6H_2O

By Stoichiometry of the reaction:

2 moles of ethane produces 6 moles of water

So, 0.513 moles of ethane will produce = \frac{6}{2}\times 0.513=1.54mol of water

Hence, the moles of water produced are 1.54 moles.

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The volume and amount of gas are constant in a tire. The initial pressure and temperature are 1.82 atm and 293 K. At what temper
vladimir1956 [14]

Answer:

When the pressure increases to 2.35 atm, the temperature will increase to 378 K

Explanation:

Step 1: Data given

The initial pressure = 1.82 atm

The initial temperature = 293 K

The pressure will be increased to 2.35 atm

Step 2: Calculate the new temperature

P1/T1 = P2/T2

⇒with P1 = the initial pressure = 1.82 atm

⇒with T1 = the initial temperature = 293 K

⇒with P2 = the increased pressure = 2.35 atm

⇒with T2 = the new temperature = TO BE DETERMINED

1.82atm / 293 K = 2.35 atm / T2

T2 = 2.35 atm / (1.82 atm/293 K)

T2 = 2.35 / 0.0062116

T2 = 378 K

When the pressure increases to 2.35 atm, the temperature will increase to 378 K

4 0
3 years ago
1. A container holds four times as many moles of CO2 as O2. If the total pressure in the container is 20. atm,
Hitman42 [59]

Answer:

Partial pressure of CO2 = 16 atm

Explanation:

Total number of moles of gases = 4+1 = 5 moles

Mole fraction of CO2 = 4/5

Partial pressure of CO2 = mole fraction of CO2 × total pressure

Partial pressure of CO2 = (4/5) × 20

Partial pressure of CO2 = 16 atm

7 0
3 years ago
The molar mass of Cr(OH)2 is:
son4ous [18]

The molar mass of Cr(OH)_2 is 86.02 g/mole .

<h3><u> Explanation:</u> </h3>

The molar mass of a chemical compound is represented as the mass of a unit of that compound separated by the number of substances in that unit, measured in moles. The molar mass is a volume, not molecular, the property of a substance.

The molar mass is a percentage of various examples of the compound, which usually change in mass due to the appearance of isotopes.

From the below attached table, the Molar mass of Cr(OH)_2 is 86.0108 g/mol.

3 0
3 years ago
How is the energy that is carried in an ATP molecule released to provide usable energy?
Irina18 [472]
The bond holding the last phosphate group breaks that is why <span> is the energy that is carried in an ATP molecule released to provide usable energy.</span>
3 0
3 years ago
Read 2 more answers
A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H2O2 w
Stels [109]

Answer:

see explanation below

Explanation:

First to all, this is a redox reaction, and the reaction taking place is the following:

2KMnO4 + 3H2SO4 + 5H2O2 -----> 2MnSO4 + K2SO4 + 8H2O + 5O2

According to this reaction, we can see that the mole ratio between the peroxide and the permangante is 5:2. Therefore, if the titration required 21.3 mL to reach the equivalence point, then, the moles would be:

MhVh = MpVp

h would be the hydrogen peroxide, and p the permanganate.

But like it was stated before, the mole ratio is 5:2 so:

5MhVh = 2MpVp

Replacing moles:

5nh = 2MpVp

Now, we just have to replace the given data:

nh = 2MpVp/5

nh = 2 * 1.68 * 0.0213 / 5

nh = 0.0143 moles

Now to get the mass, we just need the molecular mass of the peroxide:

MM = 2*1 + 2*16 = 34 g/mol

Finally the mass:

m = 0.0143 * 34

m = 0.4862 g

8 0
3 years ago
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