Chapter 16: Problem 1
How does a developing fetus get oxygen in the womb?
Short Answer
Step by step solution
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chapter 16: Problem 1
How does a developing fetus get oxygen in the womb?
These are the key concepts you need to understand to accurately answer the question.
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Get started for freeConsider the reaction: \begin{equation}2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) \Longrightarrow 2 \operatorname{NOBr}(g) \atop K_{\mathrm{p}}=28.4 \mathrm{at} 298 \mathrm{K}\end{equation} In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of \(\mathrm{Br}_{2}\) is 126 torr. What is the partial pressure of NOBr in this mixture?
Consider the reaction: \begin{equation}\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g)\end{equation} An equilibrium mixture of this reaction at a certain temperature has \([\mathrm{CO}]=0.105 \mathrm{M},\left[\mathrm{H}_{2}\right]=0.114 \mathrm{M},\) and \(\left[\mathrm{CH}_{3} \mathrm{OH}\right]=0.185 \mathrm{M} .\) What is the value of the equilibrium constant \(\left(K_{\mathrm{c}}\right)\) at this temperature?
Consider the reaction and the associated equilibrium constant: $$a \mathrm{A}(g)+b \mathrm{B}(g) \rightleftharpoons c \mathrm{C}(g) \quad K_{\mathrm{c}}=5.0$$ Find the equilibrium concentrations of \(\mathrm{A}, \mathrm{B},\) and \(\mathrm{C}\) for each value of \(a\) \(b,\) and \(c\) . Assume that the initial concentrations of \(\mathrm{A}\) and \(\mathrm{B}\) are each 1.0 \(\mathrm{M}\) and that no product is present at the beginning of the reaction. \begin{equation} \begin{array}{l}{\text { a. } a=1 ; b=1 ; c=2} \\ {\text { b. } a=1 ; b=1 ; c=1} \\ {\text { c. } a=2 ; b=1 ; c=1 \text { (set up equation for } x ; \text { don't solve) }}\end{array} \end{equation}
What is the effect of a change in concentration of a reactant or product on a chemical reaction initially at equilibrium?
Calculate \(K_{\mathrm{c}}\) for each reaction. \begin{equation}\begin{array}{l}{\text { a. } \mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g) \quad K_{c}=5.9 \times 10^{-3}(\mathrm{at} 298 \mathrm{K})} \\ {\text { b. } \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) \quad K_{\mathrm{c}}=3.7 \times 10^{8}(\mathrm{at} 298 \mathrm{K})} \\ {\text { c. } \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) \quad K_{\mathrm{c}}=4.10 \times 10^{-31}(\mathrm{at} 298 \mathrm{K})}\end{array}\end{equation}
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