For the following reaction, if the rate of appearance of HCI(g) is 0.0117 M/s, what is the rate of disappearance of H2O (g) ? SiCl«(g) + 2 H2O (g) →2 SiO2(s) + 4 HCI(g) a. 0.0234 M/s b. 0.0117 M/s c. 0.0058 M/s d. 0.0704 M/s e. 0.0351 M/s
For the following reaction, if the rate of appearance of HCI(g) is 0.0117 M/s, what is the rate of disappearance of H2O (g) ? SiCl«(g) + 2 H2O (g) →2 SiO2(s) + 4 HCI(g) a. 0.0234 M/s b. 0.0117 M/s c. 0.0058 M/s d. 0.0704 M/s e. 0.0351 M/s
Chemistry
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Reaction Rate Problem
#### Problem Statement:
For the following reaction, if the rate of appearance of HCl(g) is 0.0117 M/s, what is the rate of disappearance of H₂O(g)?
\[ \text{SiCl}_4(g) + 2 \text{H}_2\text{O}(g) \rightarrow 2 \text{SiO}_2(s) + 4 \text{HCl}(g) \]
#### Options:
a. \( 0.0234 \, \text{M/s} \)
b. \( 0.0117 \, \text{M/s} \)
c. \( 0.0058 \, \text{M/s} \)
d. \( 0.0704 \, \text{M/s} \)
e. \( 0.0351 \, \text{M/s} \)
#### Explanation:
In this chemical reaction, stoichiometry can be used to relate the rate of disappearance of one reactant to the rate of appearance of another product. The balanced chemical equation given is:
\[ \text{SiCl}_4(g) + 2 \text{H}_2\text{O}(g) \rightarrow 2 \text{SiO}_2(s) + 4 \text{HCl}(g) \]
From the equation, we see that 2 moles of H₂O produce 4 moles of HCl. Therefore, the rate of disappearance of H₂O is half the rate of appearance of HCl.
Rate of disappearance of H₂O \( = \frac{\text{Rate of appearance of } \text{HCl}}{2} \)
Given the rate of appearance of HCl is \( 0.0117 \, \text{M/s} \), the rate of disappearance of H₂O is:
\[ \text{Rate of disappearance of H₂O} = \frac{0.0117}{2} = 0.00585 \, \text{M/s} \]
None of the given options exactly matches 0.00585 M/s. Therefore, an option closest to this value (rounding or consideration of significant figures might result in one of the options). The correct answer appears to be:
\[ \boxed{0.0058 \, \text{M/s}} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F48deb947-3d41-43de-ac43-bef03e01cc59%2F99668968-5eb1-4e1c-be59-913ec2cebff3%2Fi5ir217.png&w=3840&q=75)
Transcribed Image Text:### Reaction Rate Problem
#### Problem Statement:
For the following reaction, if the rate of appearance of HCl(g) is 0.0117 M/s, what is the rate of disappearance of H₂O(g)?
\[ \text{SiCl}_4(g) + 2 \text{H}_2\text{O}(g) \rightarrow 2 \text{SiO}_2(s) + 4 \text{HCl}(g) \]
#### Options:
a. \( 0.0234 \, \text{M/s} \)
b. \( 0.0117 \, \text{M/s} \)
c. \( 0.0058 \, \text{M/s} \)
d. \( 0.0704 \, \text{M/s} \)
e. \( 0.0351 \, \text{M/s} \)
#### Explanation:
In this chemical reaction, stoichiometry can be used to relate the rate of disappearance of one reactant to the rate of appearance of another product. The balanced chemical equation given is:
\[ \text{SiCl}_4(g) + 2 \text{H}_2\text{O}(g) \rightarrow 2 \text{SiO}_2(s) + 4 \text{HCl}(g) \]
From the equation, we see that 2 moles of H₂O produce 4 moles of HCl. Therefore, the rate of disappearance of H₂O is half the rate of appearance of HCl.
Rate of disappearance of H₂O \( = \frac{\text{Rate of appearance of } \text{HCl}}{2} \)
Given the rate of appearance of HCl is \( 0.0117 \, \text{M/s} \), the rate of disappearance of H₂O is:
\[ \text{Rate of disappearance of H₂O} = \frac{0.0117}{2} = 0.00585 \, \text{M/s} \]
None of the given options exactly matches 0.00585 M/s. Therefore, an option closest to this value (rounding or consideration of significant figures might result in one of the options). The correct answer appears to be:
\[ \boxed{0.0058 \, \text{M/s}} \]
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