What do you think the tomato seeds might represent in "In Response to Executive Order 9066"? Think about · what Denise calls them · where they will not grow · what the speaker says Denise will do when they ripen

Rewrite the sentence. Replace the underlined word or words with a vocabulary word or a form of a vocabulary word.

When Anna fell, she skinned her knee and broke a few $\mathrm{\underline{small}}$ $\mathrm{\underline{blood}}$ $\mathrm{\underline{vessels}}$.

Solve. Write the answer in scientific notation.

Use the information in the article at the right. Find the number of seeds released by the lodgepole pine trees for each surviving seedling.

Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide $\left(\mathrm{NO}_2\right)$, a dark-brown gas:

$$2 \mathrm{NO}(g)+\mathrm{O}_2(g) \longrightarrow 2 \mathrm{NO}_2(g)$$

In one experiment, $0.886$ mole of $\mathrm{NO}$ is mixed with $0.503$ mole of $\mathrm{O}_2$. Determine which of the two reactants is the limiting reactant. Calculate also the number of moles of $\mathrm{NO}_2$ produced.

Two enthalpy of formation equations, a and b, combine to form the equation for the reaction of nitrogen oxide and oxygen. The product of the reaction is nitrogen dioxide: $\mathrm{NO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{NO}_{2}(\mathrm{g}) \Delta H_{\mathrm{rxn}}^{\circ}=-58.1 \mathrm{kJ}$. $\frac{1}{2} N_{2}(g)+O_{2}(g) \rightarrow N O_{2}(g) \Delta H_{f}^{\circ}=?$ What is $\Delta H_{f}^{\circ}$?

A harbor buoy bobs up and down with the waves. The distance between the highest and lowest points is 4 feet. The buoy moves from its highest point to its lowest point and back to its highest point every 10 seconds. What is the height of the buoy after 12 seconds?

What does the phrase “no matter how lonely” (l. $13$) suggest about the speaker’s assumptions regarding her audience? What does the phrase suggest about the poem’s purpose? How does that description link to the opening sentence?

Use the information in the table to find the 16. Short Response Reggie started constant rate of change.

$$\begin{matrix} \text{Number of Apples} & \text{3} & \text{7} & \text{11}\\ \text{Number of Seeds} & \text{30} & \text{70} & \text{110}\\ \end{matrix}$$

A. $\frac{10}{1}$, B. $\frac{1}{10}$, C. $\frac{40}{4}$, D. $\frac{4}{40}$.

Link 2 is isolated from a kinematic diagram and shown. The link is rotating counterclockwise at a rate of $300 \mathrm{rpm}$. Determine the velocity of points $A$ and $B$. Use $\gamma=50^{\circ}$ and $\beta=60^{\circ}$.

Perform the indicated operation in trigonometric form. Write the solution in standard form. Round approximate constants to the nearest ten-thousandth. $\frac{(2-2 i \sqrt{3})(1-i \sqrt{3})}{4 \sqrt{3}+4 i}$

Discriminate between immediate hypersensitivity and delayed-type hypersensitivity with respect to antigens and immune effectors.

Nitrogen monoxide reacts with oxygen to give nitrogen dioxide:

$$\begin{align*} 2 NO ( g )+ O _2( g ) \rightarrow 2 NO _2( g ) \end{align*}$$

(a) Place the three gases in order of increasing rms speed at $298 K$.

At temperatures below $500 \mathrm{~K}$, the reaction between carbon monoxide and nitrogen dioxide

$$\begin{align*} \mathrm{CO}(\mathrm{g})+\mathrm{NO}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})+\mathrm{NO}(\mathrm{g}) \end{align*}$$

has the following rate equation: Rate $=k\left[\mathrm{NO}_2\right]^2$. Which of the three mechanisms suggested here best agrees with the experimentally observed rate equation? Mechanism 1 Single, elementary step

$$\begin{align*} \mathrm{NO}_2+\mathrm{CO} \rightarrow \mathrm{CO}_2+\mathrm{NO} \end{align*}$$

Mechanism 2 Two steps
Slow $\quad \mathrm{NO}_2+\mathrm{NO}_2 \rightarrow \mathrm{NO}_9+\mathrm{NO}$
Fast $\quad \mathrm{NO}_3+\mathrm{CO} \rightarrow \mathrm{NO}_2+\mathrm{CO}_2$
Mechanism 3 Two steps
Slow $\quad \mathrm{NO}_2 \rightarrow \mathrm{NO}+\mathrm{O}$
Fast $\quad \mathrm{CO}+\mathrm{O} \rightarrow \mathrm{CO}_2$

The rate of the reaction

$$\mathrm { NO } _ { 2 } ( g ) + \mathrm { CO } ( g ) \longrightarrow \mathrm { NO } ( g ) + \mathrm { CO } _ { 2 } ( g )$$

depends only on the concentration of nitrogen dioxide at temperatures below $225 ^ { \circ } \mathrm { C }.$ At a temperature below $225 ^ { \circ } \mathrm { C } ,$ the following data were collected:

$$\text {Time(s)} \quad \quad [ \mathrm { NO } _ { 2 } ] ( \mathrm { mol } / \mathrm { L } )$$

$$\begin{array} { r r } { 0 } \quad \quad \quad \quad { 0.500 } \\ { 1.20 \times 10 ^ { 3 } } \quad \quad \quad \quad { 0.444 } \\ { 3.00 \times 10 ^ { 3 } } \quad \quad \quad \quad { 0.381 } \\ { 4.50 \times 10 ^ { 3 } } \quad \quad \quad \quad { 0.340 } \\ { 9.00 \times 10 ^ { 3 } } \quad \quad \quad \quad { 0.250 } \\ { 1.80 \times 10 ^ { 4 } } \quad \quad \quad \quad { 0.174 } \end{array}$$

Determine the integrated rate law, the differential rate law, and the value of the rate constant at this temperature. Calculate $\left[ \mathrm { NO } _ { 2 } \right]$ at $2.70 \times 10 ^ { 4 }\ \mathrm { s }$ after the start of the reaction.