Thanks for the help earlier
My question
Silicon tetrachloride (SiCl4) can be prepared by heating Si in chlorine gas:
Si + 2Cl2 yields SiCl4
In one reaction 0.507 mole of SiCl4 is produced. How many moles of molecular chlorine were used in the reaction?
Ok is it makeing reference to the Chlorine in reactants or products
also the answer in the back of the book says 1.01 mol of Cl2 so I guess its the reactants it makeing reference to
Now I am kind of confused because I thought there were 2 moles of carbon in the reactants
I thought I was suppose to do something like this
1 mole of Si is stoichiometrically equivalent to 2 moles of Cl2
from which I can set up a fraction but apparently that is wrong...
I kind of don't know how to start this problem can you help me thanks
Silicon tetrachloride (SiCl4) can be prepared by heating Si in chlorine gas:
Si + 2Cl2 yields SiCl4
In one reaction 0.507 mole of SiCl4 is produced. How many moles of molecular chlorine were used in the reaction?
Ok is it makeing reference to the Chlorine in reactants or products
It's making reference to moles Cl2 in the reactants. That's the only place MOLECULAR chlorine is found. There is no molecular chlorine in SiCl4
also the answer in the back of the book says 1.01 mol of Cl2 so I guess its the reactants it makeing reference to
Again, yes. 0.507 moles SiCl4 x (2 moles Cl2/1 mole SiCl4) = 0.507 X (2/1) = 1.01 moles.
Now I am kind of confused because I thought there were 2 moles of carbon in the reactants
There is no carbon in the entire reaction. The C you have there goes with the l to make Cl which is chlorine.
I thought I was suppose to do something like this
1 mole of Si is stoichiometrically equivalent to 2 moles of Cl2
from which I can set up a fraction but apparently that is wrong.
The process is ok and the answer you get is the correct answer but you arrived at it incorrectly. The question is about SiCl4 and Cl2 and has nothing to do with Si in this part of the problem. See the earlier fraction I set up and you get 0.507 x 2 = 1.01 moles Cl2.
I kind of don't know how to start this problem can you help me thanks
* Chemistry - Kate, Saturday, July 3, 2010 at 10:38pm
Ok apparently its just the mole ratio 2:1 from the coefficents
so I just do 2(.507) to get my answer but how come I ignoered the coeficent of the Si in ther reaction?
The problem is about the product, SiCl4, and not about Si. It follows from the stoichiometry that 1 mole SiCl4 = 1 mole Si; therefore, if you had stoichiometric quantities, then 0.507 moles SiCl4 would have begun with 0.507 moles Si.
Ok apparently its just the mole ratio 2:1 from the coefficents
so I just do 2(.507) to get my answer but how come I ignoered the coeficent of the Si in ther reaction?
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The only one answer
Coefisient : 1 --> 2
x0.507 ----> 0.507 --> 1.014 gram
1.014 gram must be rounded
in 3 SCIENTIFIC NUMBER ---> 1.01 GRAM
MUST BE 3 IMPORTANT NUMBER
you have the mole : .507
so
cl2 :cl2 ::sicl4:sicl4
2 :x ::1 :.5o7
x*1=2*.507
x= 1.01 mole of cl2
Of course, I'm here to help! Let's break it down step by step.
The balanced equation for the reaction is:
Si + 2Cl2 → SiCl4
First, let's identify what we know:
- The amount of SiCl4 produced is 0.507 moles.
Now, we want to find the number of moles of Cl2 used. Since the coefficient of Cl2 in the balanced equation is 2, we can assume that the ratio of moles of Cl2 to moles of SiCl4 is also 2:1.
So, if we have 0.507 moles of SiCl4, we can set up a proportion:
(0.507 moles SiCl4) / (1 mole Cl2) = (x moles SiCl4) / (2 moles Cl2)
Solving the proportion:
0.507 / 1 = x / 2
x = (0.507 * 2) / 1
x = 1.014 moles Cl2
Therefore, the number of moles of Cl2 used in the reaction is approximately 1.014 moles, which is close to the answer in the back of the book (1.01 mol).
Hope that helps! Let me know if you have any further questions or need more clarification.
Of course! I'll be happy to help you with this chemistry problem.
The balanced chemical equation given for the reaction is:
Si + 2Cl2 → SiCl4
Looking at the equation, you are correct that 1 mole of Si is stoichiometrically equivalent to 2 moles of Cl2. This means that for every 1 mole of Si consumed, you need 2 moles of Cl2 to react completely.
To find how many moles of Cl2 were used in the reaction, you need to determine the moles of SiCl4 produced and then use the stoichiometry of the balanced equation to find the moles of Cl2.
Given that 0.507 moles of SiCl4 were produced, we can use the stoichiometry of the balanced equation to find the corresponding moles of Cl2.
Since 1 mole of Si reacts with 2 moles of Cl2, you can set up a proportion like this:
(0.507 mol SiCl4) / (1 mol SiCl4) = (x mol Cl2) / (2 mol Cl2)
Simplifying the proportion:
0.507 mol SiCl4 = (x mol Cl2) / 2
Rearranging the equation to solve for x:
x mol Cl2 = 0.507 mol SiCl4 * 2
x mol Cl2 = 1.014 mol Cl2
Therefore, the number of moles of Cl2 used in the reaction is 1.014 mol Cl2.
It seems there was an error in the answer provided in the back of the book. The correct answer should be 1.014 mol Cl2, not 1.01 mol Cl2.
I hope this clears up your confusion! Let me know if there's anything else I can assist you with.