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erastova [34]
2 years ago
15

IF CORRECT YOU WILL GET BRAINLIEST

Chemistry
2 answers:
Dahasolnce [82]2 years ago
5 0

Answer:

okk

Explanation:

lol jajajjajjajjaajajajaja

Scorpion4ik [409]2 years ago
3 0

Answer:

C 5 mol A; 6 mol B

Explanation:

eto po answer ko sana makatulong

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How many liters of C3H6O are present in a sample weighing 25.6 grams?
lawyer [7]

To Find :

Number of moles of C₃H₆O present in a sample weighing 25.6 grams.

Solution :

Molecular mass of C₃H₆O is :

M = (6×12) + (6×1) + (16×1) grams

M = 94 grams/mol

We know, number of moles of 25.6 grams of C₃H₆O is :

n = \dfrac{Given \ Mass \ Of \ C_3H_6O }{Molar\ Mass \ Of \ C_3H_6O }\\\\n = \dfrac{25.6}{94}\ mole\\\\n = 0.27 \ mole

Hence, this is the required solution.

4 0
3 years ago
Vinegar is a solution of acetic acid (the solute) in water (the solvent) with a solution density of 1010 g/L. If vinegar is 0.80
Damm [24]

Answer:

4.8 %

Explanation:

We are asked the concentration in % by mass, given the molarity of the solution and its density.

0.8 molar solution means that we have 0.80 moles of acetic acid in 1 liter of solution. If we convert the moles of acetic acid to grams, and the 1 liter solution to grams, since we are given the density of solution, we will have the values necessary to calculate the % by mass:

MW acetic acid = 60.0 g/mol

mass acetic acid (the solute) = 0.80 mol x 60 g / mol = 48.00 g

mass of solution = 1000 cm³ x 1.010 g/ cm³      (1l= 1000 cm³)

                            = 1010 g

% (by mass) = 48.00 g/ 1010 g  x 100 = 4.8 %

6 0
3 years ago
What is the difference between a theory and a law?​
kondaur [170]

Answer:

theory is diffrent from law

Explanation:

a Theory can never be proven to be true nd a law can usually be expressed

3 0
3 years ago
Which of the following is a chemical property?
TEA [102]
The answer to this question is A
6 0
3 years ago
Read 2 more answers
Ammonia gas will react with oxygen gas to yield nitrogen monoxide gas and water vapor.
ruslelena [56]

Answer:

a) <u>0.168 moles O2</u>

<u>b) </u> <u>9.50 grams O2</u>

<u>c) 0.01662 kg NO</u>

<u>d)</u>88.9 %

Explanation:

Step 1: Data given

Molar mass of NH3 = 17.03 g/mol

Molar mass of O2 = 32 g/mol

Molar mass of NO = 30.01 g/mol

Molar mass of H2O = 18.02 g/mol

Step 2: The balanced equation:

4NH3 + 5O2 → 4NO + 6H2O

a. How many moles of ammonia will react with 6.73g of oxygen?

Calculate moles of oxygen = mass O2/ molar mass O2

moles oxygen =  6.73 grams / 32.00 g/mol = 0.210 moles

Calculate moles of NH3

For 4 moles of NH3 we need 5 moles O2 to produce 4 moles NO and 6 moles H2O

For 0.210 moles O2 we need 4/5 *0.210 = <u>0.168 moles O2</u>

<u />

b. If 6.42g of water is produced, how many grams of oxygen gas reacted?

Calculate moles of H2O = 6.42 grams / 18.02 g/mol = 0.356 moles

Calculate moles of O2:

For 4 moles of NH3 we need 5 moles O2 to produce 4 moles NO and 6 moles H2O

For 0.356 moles H2O we'll need 5/6 * 0.356 = 0.297 moles O2

Calculate mass of O2 = moles O2 * molar mass O2

Mass O2 = 0.297 moles O2 * 32.00 g/mol =  <u>9.50 grams O2</u>

c. If the reaction uses up 9.43105 g of ammonia, how many kilograms of nitrogen monoxide will be formed?

Calculate moles of ammonia = 9.43105 grams / 17.03 g/mol =0.5538 moles

Calculate moles of NO:

For 4 moles of NH3 we need 5 moles O2 to produce 4 moles NO and 6 moles H2O

For 0.5538 moles of NH3 we'll have 0.5538 moles NO

Calculate mass of NO

Mass NO = 0.5538 moles * 30.01 g/mol = 16.62 grams = <u>0.01662 kg NO</u>

<u />

<u />

d. When 2.51 g of ammonia react with 3.76 g of oxygen, 2.27 g of water vapor are produced. What is the percentage yield of water?

<em>Calculate moles of NH3</em> = 2.51 grams / 17.03 g/mol = 0.147 moles

<em>Calculate moles of O2 </em>= 3.76 grams / 32 g/mol = 0.118 moles

<em>Determine the limiting reactant</em>

O2 is the limiting reactant, it will completely be consumed (0.118 moles)

NH3 is in excess. There will react 4/5 * 0.118 = 0.0944 moles

There will remain 0.147 - 0.0944 = 0.0526 moles

<em>Calculate moles H2O</em>: For 0.118 moles O2 we'll have 6/5 * 0.118 = 0.1416 moles H2O

<em>Calculate mass H2O</em> = 0.1416 moles * 18.02 g/mol = 2.552 grams H2O

<em>Calculate % yield</em> = (2.27/2.552)*100 % = <u>88.9 %</u>

4 0
3 years ago
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