Answer:
0.86 moles H₂O
Explanation:
To solve this problem, it is important to first determine the balanced chemical equation. The balanced equation is necessary as it will provide the mole-to-mole ratio needed to convert between moles O₂ and moles H₂O.
The unbalanced equation:
C₈H₁₈ (l) + O₂ (g) ---> CO₂ (g) + H₂O (g)
<u>Reactants:</u> 8 carbon, 18 hydrogen, 2 oxygen
<u>Products:</u> 1 carbon, 2 hydrogen, 3 oxygen
As you can see, the equation is not balanced because there are unequal amounts of each element on both sides. Balancing the equation is a matter of guessing-and-checking to see which combination of coefficients work.
The balanced equation:
2 C₈H₁₈ (l) + 25 O₂ (g) ---> 16 CO₂ (g) + 18 H₂O (g)
<u>Reactants:</u> 16 carbon, 36 hydrogen, 50 oxygen
<u>Products:</u> 16 carbon, 36 hydrogen, 50 oxygen
Now that the equation is balanced, we can use the coefficients of O₂ and H₂O to construct our mole-to-mole ratio and perform our conversion. The final answer should have 2 sig figs to match the given value (1.2 moles). The state of matter is most likely not necessary to include in your final answer.
1.2 moles O₂ 18 moles H₂O
--------------------- x ----------------------- = 0.86 moles H₂O
25 moles O₂
<u>Answer:</u> The value of
for the surrounding when given amount of hydrogen gas is reacted is -31.02 J/K
<u>Explanation:</u>
Entropy change is defined as the difference in entropy of all the product and the reactants each multiplied with their respective number of moles.
The equation used to calculate entropy change is of a reaction is:
![\Delta S^o_{rxn}=\sum [n\times \Delta S^o_{(product)}]-\sum [n\times \Delta S^o_{(reactant)}]](https://tex.z-dn.net/?f=%5CDelta%20S%5Eo_%7Brxn%7D%3D%5Csum%20%5Bn%5Ctimes%20%5CDelta%20S%5Eo_%7B%28product%29%7D%5D-%5Csum%20%5Bn%5Ctimes%20%5CDelta%20S%5Eo_%7B%28reactant%29%7D%5D)
For the given chemical reaction:

The equation for the entropy change of the above reaction is:
![\Delta S^o_{rxn}=[(2\times \Delta S^o_{(HF(g))})]-[(1\times \Delta S^o_{(H_2(g))})+(1\times \Delta S^o_{(F_2(g))})]](https://tex.z-dn.net/?f=%5CDelta%20S%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%5CDelta%20S%5Eo_%7B%28HF%28g%29%29%7D%29%5D-%5B%281%5Ctimes%20%5CDelta%20S%5Eo_%7B%28H_2%28g%29%29%7D%29%2B%281%5Ctimes%20%5CDelta%20S%5Eo_%7B%28F_2%28g%29%29%7D%29%5D)
We are given:

Putting values in above equation, we get:
![\Delta S^o_{rxn}=[(2\times (173.78))]-[(1\times (130.68))+(1\times (202.78))]\\\\\Delta S^o_{rxn}=14.1J/K](https://tex.z-dn.net/?f=%5CDelta%20S%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%28173.78%29%29%5D-%5B%281%5Ctimes%20%28130.68%29%29%2B%281%5Ctimes%20%28202.78%29%29%5D%5C%5C%5C%5C%5CDelta%20S%5Eo_%7Brxn%7D%3D14.1J%2FK)
Entropy change of the surrounding = - (Entropy change of the system) = -(14.1) J/K = -14.1 J/K
We are given:
Moles of hydrogen gas reacted = 2.20 moles
By Stoichiometry of the reaction:
When 1 mole of hydrogen gas is reacted, the entropy change of the surrounding will be -14.1 J/K
So, when 2.20 moles of hydrogen gas is reacted, the entropy change of the surrounding will be = 
Hence, the value of
for the surrounding when given amount of hydrogen gas is reacted is -31.02 J/K
A. Dalton's theory that atoms could not be divided was incorrect
Hello!
A) H<span>ow many grams of hydrogen are necessary to react completely with 50.0g of nitrogen in the above reaction?
The balanced chemical reaction is the following one:
N</span>
₂(g) + 3H₂(g) → 2NH₃(g)To calculate the amount of hydrogen necessary we will use the following conversion factor to go from grams of nitrogen to grams of hydrogen:

So, 10,7950
grams of H₂ are required to react with 50 g of nitrogen
<span>B) How many grams of ammonia are produced in the reaction from the previous problem?
</span>The balanced chemical reaction again is the following one:
N₂ + 3H₂ → 2NH₃To calculate the amount of ammonia produced we will use the following conversion factor to go from grams of nitrogen to grams of ammonia:

So, 60,7968
grams of NH₃ are produced from 50 g of nitrogen
C) <span>How many grams of silver chloride are produced from 5.0g of silver nitrate reacting with an excess of barium chloride?
The balanced chemical equation for the reaction is the following one:
2AgNO</span>
₃ + BaCl₂ → 2AgCl + Ba(NO₃)₂
To calculate the mass of Silver Chloride produced we will use the following conversion factor to go from grams of Silver Nitrate to grams of Silver Chloride:

So,
4,219 g of AgCl are produced from the reaction of 5 g of AgNO₃
D) <span>How much barium chloride is necessary to react with the silver nitrate in the previous problem?
</span>The balanced chemical equation for the reaction is the following one:
2AgNO₃ + BaCl₂ → 2AgCl + Ba(NO₃)₂
To calculate the mass of Barium Chloride necessary we will use the following conversion factor to go from grams of Silver Nitrate to grams of Barium Chloride:

So,
3,08 g of BaCl₂ are produced from the reaction of 5 g of AgNO₃
Have a nice day!