NiO is to be reduced to nickel metal in an industrial process by use of the reaction NiO (s) + CO(g) = Ni(s) + CO₂(g). At 1600 K the equilibrium constant for the reaction is K₂ = 6.0 x 10². Part A A 42.0-L reactor at 1600 K is charged with 50.0 g of NiO(s) and 1.10 atm of CO(g). After equilibrium is reached, what is the partial pressure of CO₂(g) in the reactor? Express your answer in atmospheres to two significant figures. P(CO₂) = Submit Part B m= 195] ΑΣΦ Submit Request Answer What mass of Ni(s) is produced in the reaction in part (a)? Express your answer in grams to two significant figures. ΨΕΙ ΑΣΦ 4 → Request Answer ? ? g atm
NiO is to be reduced to nickel metal in an industrial process by use of the reaction NiO (s) + CO(g) = Ni(s) + CO₂(g). At 1600 K the equilibrium constant for the reaction is K₂ = 6.0 x 10². Part A A 42.0-L reactor at 1600 K is charged with 50.0 g of NiO(s) and 1.10 atm of CO(g). After equilibrium is reached, what is the partial pressure of CO₂(g) in the reactor? Express your answer in atmospheres to two significant figures. P(CO₂) = Submit Part B m= 195] ΑΣΦ Submit Request Answer What mass of Ni(s) is produced in the reaction in part (a)? Express your answer in grams to two significant figures. ΨΕΙ ΑΣΦ 4 → Request Answer ? ? g atm
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**NiO Reduction to Nickel Metal in Industrial Processes**
**Reaction:**
\[ \text{NiO(s)} + \text{CO(g)} \rightarrow \text{Ni(s)} + \text{CO}_2\text{(g)} \]
At 1600 K, the equilibrium constant for the reaction is \( K_p = 6.0 \times 10^2 \).
**Part A:**
A 42.0-L reactor at 1600 K is charged with 50.0 g of \(\text{NiO(s)}\) and 1.10 atm of \(\text{CO(g)}\). After equilibrium is reached, what is the partial pressure of \(\text{CO}_2\text{(g)}\) in the reactor?
*Express your answer in atmospheres to two significant figures.*
\[ P(\text{CO}_2) = \_\_\_ \, \text{atm} \]
*Submit Button*
**Part B:**
What mass of \(\text{Ni(s)}\) is produced in the reaction in part (a)?
*Express your answer in grams to two significant figures.*
\[ m = \_\_\_ \, \text{g} \]
*Submit Button*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1205cd08-0e41-4ad8-bd1c-6b97372ee2c1%2F836cfe12-5a7f-42ef-9972-4e1173127322%2Flb9d40o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**NiO Reduction to Nickel Metal in Industrial Processes**
**Reaction:**
\[ \text{NiO(s)} + \text{CO(g)} \rightarrow \text{Ni(s)} + \text{CO}_2\text{(g)} \]
At 1600 K, the equilibrium constant for the reaction is \( K_p = 6.0 \times 10^2 \).
**Part A:**
A 42.0-L reactor at 1600 K is charged with 50.0 g of \(\text{NiO(s)}\) and 1.10 atm of \(\text{CO(g)}\). After equilibrium is reached, what is the partial pressure of \(\text{CO}_2\text{(g)}\) in the reactor?
*Express your answer in atmospheres to two significant figures.*
\[ P(\text{CO}_2) = \_\_\_ \, \text{atm} \]
*Submit Button*
**Part B:**
What mass of \(\text{Ni(s)}\) is produced in the reaction in part (a)?
*Express your answer in grams to two significant figures.*
\[ m = \_\_\_ \, \text{g} \]
*Submit Button*
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