ct so d ▼ Hydrogen is used as a rocket fuel because it is very light and reacts explosively and completely with oxygen. For the combustion reaction what is the likely magnitude of the equilibrium constant K? ▸ View Available Hint(s) OK <10 3 O 10-³ 10³ Submit Part B 2H₂(g) + O₂(g) = 2H₂O(g) The industrial production of lime (CaO) from calcium carbonate is accomplished via the following reaction: CaCO3(s) CaO(s) + CO₂(g) Given the following data: what can be said about this reaction? ▸ View Available Hint(s) = Temperature (K) 298 1200 O Lower temperatures result in more lime formation. The reaction makes more lime at higher temperatures. O The reaction goes to completion at 1200 K. O The equilibrium lies far to the right at room temperature. K 1.93 x 10-23 1.01
ct so d ▼ Hydrogen is used as a rocket fuel because it is very light and reacts explosively and completely with oxygen. For the combustion reaction what is the likely magnitude of the equilibrium constant K? ▸ View Available Hint(s) OK <10 3 O 10-³ 10³ Submit Part B 2H₂(g) + O₂(g) = 2H₂O(g) The industrial production of lime (CaO) from calcium carbonate is accomplished via the following reaction: CaCO3(s) CaO(s) + CO₂(g) Given the following data: what can be said about this reaction? ▸ View Available Hint(s) = Temperature (K) 298 1200 O Lower temperatures result in more lime formation. The reaction makes more lime at higher temperatures. O The reaction goes to completion at 1200 K. O The equilibrium lies far to the right at room temperature. K 1.93 x 10-23 1.01
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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![**Equilibrium Constant in Chemical Reactions**
**For a reaction**
\[ aA + bB \rightleftharpoons cC + dD \]
the equilibrium constant \( K \) is defined as the ratio of products to reactants at equilibrium:
\[ K = \frac{[C]^c [D]^d}{[A]^a [B]^b} \]
Because \( K \) represents the ratio of products to reactants, the magnitude of \( K \) is an indicator of the levels of products and reactants present when the reaction is at equilibrium. Some chemical reactions proceed almost fully to product, whereas other chemicals hardly react with each other at all, or react so as to have significant amounts of both reactants and products at equilibrium.
**Hydrogen as a Rocket Fuel**
Hydrogen is used as a rocket fuel because it is very light and reacts explosively and completely with oxygen. For the combustion reaction:
\[ 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \]
what is the likely magnitude of the equilibrium constant \( K \)?
- \( K < 10^{-3} \)
- \( 10^{-3} < K < 10^{3} \)
- \( K = 0 \)
- \( K > 10^{3} \)
**Part B: Industrial Production of Lime**
The industrial production of lime (CaO) from calcium carbonate is accomplished via the following reaction:
\[ \text{CaCO}_3(s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g) \]
Given the following data:
| Temperature (K) | \( K \) |
|-----------------|------------------|
| 298 | \( 1.93 \times 10^{-23} \) |
| 1200 | 1.01 |
**What can be said about this reaction?**
- Lower temperatures result in more lime formation.
- The reaction makes more lime at higher temperatures.
- The reaction goes to completion at 1200 K.
- The equilibrium lies far to the right at room temperature.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1205cd08-0e41-4ad8-bd1c-6b97372ee2c1%2F9762e6ee-3e36-4876-8890-c8b4c1a95f8e%2Fyn1myei_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Equilibrium Constant in Chemical Reactions**
**For a reaction**
\[ aA + bB \rightleftharpoons cC + dD \]
the equilibrium constant \( K \) is defined as the ratio of products to reactants at equilibrium:
\[ K = \frac{[C]^c [D]^d}{[A]^a [B]^b} \]
Because \( K \) represents the ratio of products to reactants, the magnitude of \( K \) is an indicator of the levels of products and reactants present when the reaction is at equilibrium. Some chemical reactions proceed almost fully to product, whereas other chemicals hardly react with each other at all, or react so as to have significant amounts of both reactants and products at equilibrium.
**Hydrogen as a Rocket Fuel**
Hydrogen is used as a rocket fuel because it is very light and reacts explosively and completely with oxygen. For the combustion reaction:
\[ 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \]
what is the likely magnitude of the equilibrium constant \( K \)?
- \( K < 10^{-3} \)
- \( 10^{-3} < K < 10^{3} \)
- \( K = 0 \)
- \( K > 10^{3} \)
**Part B: Industrial Production of Lime**
The industrial production of lime (CaO) from calcium carbonate is accomplished via the following reaction:
\[ \text{CaCO}_3(s) \rightleftharpoons \text{CaO}(s) + \text{CO}_2(g) \]
Given the following data:
| Temperature (K) | \( K \) |
|-----------------|------------------|
| 298 | \( 1.93 \times 10^{-23} \) |
| 1200 | 1.01 |
**What can be said about this reaction?**
- Lower temperatures result in more lime formation.
- The reaction makes more lime at higher temperatures.
- The reaction goes to completion at 1200 K.
- The equilibrium lies far to the right at room temperature.
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