Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

At \(1000^{\circ} \mathrm{C}\), the equilibrium constant for the reaction of the system \(2 \mathrm{II}_{2}(\mathrm{~g}) \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{II}_{2} \mathrm{O}(\mathrm{g})\) is very largc. This implics that (1) \(\mathrm{II}_{2} \mathrm{O}(\mathrm{g})\) is unstable at \(1000^{\circ} \mathrm{C}\) (2) \(\mathrm{II}_{2}(\mathrm{~g})\) is unstable at \(1000^{\circ} \mathrm{C}\) (3) \(\mathrm{II}_{2}\) and \(\mathrm{O}_{2}\) have very little tendency to combinc at \(1000^{\circ} \mathrm{C}\) (4) \(\mathrm{II}_{2} \mathrm{O}(\mathrm{g})\) has very little tendency to decompose into \(\mathrm{II}_{2}(\mathrm{~g})\) and \(\mathrm{O}_{2}(\mathrm{~g})\) at \(1000^{\circ} \mathrm{C}\)

Short Answer

Expert verified
The correct answer is option 4.

Step by step solution

01

Understand the Equilibrium Constant

The equilibrium constant (K) expresses the ratio of the concentrations of products to reactants at equilibrium. A very large equilibrium constant means that, at equilibrium, the concentration of the products is much higher than that of the reactants.
02

Analyze the Reaction

For the reaction \(2 \mathrm{II}_{2}(\text{g}) + \mathrm{O}_{2}(\text{g}) \rightleftharpoons 2 \mathrm{II}_{2}\mathrm{O}(\text{g})\), the large equilibrium constant indicates that the formation of \(\mathrm{II}_{2}\mathrm{O}(\text{g})\) is highly favored over the reverse reaction, which is the decomposition of \(\mathrm{II}_{2}\mathrm{O}(\text{g})\).
03

Deduce the Stability of Compounds

Since the equilibrium heavily favors the formation of \(\mathrm{II}_{2}\mathrm{O}(\text{g})\), it suggests that \(\mathrm{II}_{2}\mathrm{O}(\text{g})\) is stable and does not easily decompose back into \(\mathrm{II}_{2}(\text{g})\) and \(\mathrm{O}_{2}(\text{g})\) at \(1000^{\circ} \mathrm{C}\) (option 4).
04

Eliminate Incorrect Options

Option 1 is incorrect because \(\mathrm{II}_{2}\mathrm{O}(\text{g})\) is actually stable. Option 2 is incorrect because it doesn’t follow from the information given about the equilibrium constant. Option 3 is likewise incorrect as the high K value means \(\mathrm{II}_{2}(\text{g})\) and \(\mathrm{O}_{2}(\text{g})\) combine readily.
05

Select the Correct Option

Therefore, the correct answer is option 4: \(\mathrm{II}_{2}\mathrm{O}(\text{g})\) has very little tendency to decompose into \(\mathrm{II}_{2}(\text{g})\) and \(\mathrm{O}_{2}(\text{g})\) at \(1000^{\circ} \mathrm{C}\).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Equilibrium Constant
The equilibrium constant, symbolized as K, is a crucial concept in chemistry that quantifies the balance between products and reactants in a chemical reaction at equilibrium. The formula for the equilibrium constant is given by the ratio of the concentrations of the products to the reactants, each raised to the power of their respective stoichiometric coefficients. Mathematically, for a reaction of the form aA + bB onumber cC + dD. keep

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

At \(25^{\circ} \mathrm{C}, \mathrm{K}_{\mathrm{C}}\) for the equilibrium \(2 \mathrm{O}_{3}(\mathrm{~g}) \rightleftharpoons 3 \mathrm{O}_{2}(\mathrm{~g})\) is \(5.5 \times 10^{57}\). This explains (1) the oxidizing power of ozone (2) the absence of detectable amounts of ozone in the lower atmospherc (3) the formation of ozonc laycr in the upper atmosphcre (4) the polluting nature of ozonc

Which of the following is correct? 1) \(K_{\mathrm{a}}\) (weak acid) \(\times K_{\mathrm{b}}\) (conjugate weak base) \(=K_{\mathrm{v}}\) 2) \(K_{\mathrm{a}}\) (strong acid) \(\times K_{\mathrm{b}}\) (conjugate strong base) \(=K_{\mathrm{w}}\) 3) \(K_{\mathrm{a}}\) (weak acid) \(\times K_{\mathrm{b}}\) (weak base) \(=K_{\mathrm{T}}\) 4) \(K_{\mathrm{a}}\) (weak acid) \(\times K_{\mathrm{b}}\) (conjugate strong base) \(=K_{\mathrm{w}}\)

The equilibrium constant for the reaction \(\mathrm{Br}_{2} \rightleftharpoons\) \(2 \mathrm{Br}\) at \(500 \mathrm{~K}\) and \(700 \mathrm{~K}\) are \(1 \times 10^{\circ}\) and \(1 \times 10^{5}\), respectively. The reaction is (1) endothermic (2) exothermic (3) fast (4) slow

One mole of nitrogen was mixed with 3 moles of hydrogen in a closed 3 litre vessel. \(20 \%\) of nitrogen is converted into \(\mathrm{NH}_{3}\). Then, \(\mathrm{K}_{\mathrm{C}}\) for the \(1 / 2 \mathrm{~N}_{2}+3 / 2 \mathrm{H}_{2}\) \(\rightleftharpoons \mathrm{NH}_{3}\) is(1) \(0.36\) litre mol 1 (2) \(0.46\) litre mol (3) \(0.5 \mathrm{~mol}\) ' litre (4) \(0.2 \mathrm{~mol}^{\text {' }}\) litre

When equal volumes of the following solutions are mixed, precipitation of \(\mathrm{AgCl}\left(K_{\mathrm{pp}}=1.8 \times 10^{10}\right)\) will occur only with (1) \(10^{-4} \mathrm{M}\left(\mathrm{Ag}^{-}\right)\) and \(10^{-4} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\) (2) \(10^{-5} \mathrm{M}\left(\Lambda \mathrm{g}^{-}\right)\) and \(10^{-5} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\) (3) \(10^{-6} \mathrm{M}\left(\Lambda \mathrm{g}^{-}\right)\) and \(10^{-6} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\) (4) \(10^{-10} \mathrm{M}\left(\Lambda \mathrm{g}^{-}\right)\) and \(10^{-10} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\)

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free