Fashion PowerPoint ${ }^{(i)}$. Create a PowerPoint presentation of fashions from one decade of the 20th century. Show your presentation to the class.

For the following exercise,

Refer to as we discussed earlier.

$$\begin{array}{|c|c|c|c|c|c|c|} \hline \boldsymbol{x} & 1 & 2 & 3 & 4 & 5 & 6 \\ \hline \boldsymbol{f}(\boldsymbol{x}) & 5.1 & 6.3 & 7.3 & 7.7 & 8.1 & 8.6 \\ \hline \end{array}$$

Use the logarithmic function to find the value of the function when $x=10$.

Why do you think an initiator molecule is needed to induce the polymerization of ethylene?

In this exercise, use Euler's Method to approximate the given value of y(t) with the time step h indicated.

y(3) ; $\quad \frac{d y}{d t}=\sqrt{t+y}, \quad$ y(2.7)=5, $\quad$ h=0.05

Determine the exact function value. $\tan \frac{5 \pi}{6}$

Find the exact value of each trigonometric function.

sin 5pi/4

Determine the exact function value. $\cos \frac{5 \pi}{3}$

Ethylene $\left(C_{2} H_{4}\right)$ reacts with hydrogen to form ethane $\left(C_{2} H_{6}\right)$. $\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{g}) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{g})+\text { heat }$ How would you regulate the temperature of this equilibrium in order to accomplish each of the following? a. increase the yield of ethane b. decrease the concentration of ethylene c. Increase the amount of hydrogen in the system

During the next week, create a list of at least 10 things you could have done to conserve the water you use.

Determine the exact function value.

$$\sec \frac{5 \pi}{4}$$

Ethylene glycol (antifreeze) has a density of $1.11 \mathrm{~g} / \mathrm{cm}^3$.
a. What is the mass in $g$ of $417 \mathrm{~mL}$ of this liquid?
b. What is the volume in $L$ of $4.1 \mathrm{~kg}$ of this liquid?

Make of change on a calculator and tell how you made it. $0.659$ to $0.658$

Ethylene glycol is represented by the formula $HOCH_2CH_2OH$. Is it likely to be soluble in water? in paint thinner? Explain your answer.

Ethylene, $\mathrm{C}_2 \mathrm{H}_4$, and water react under appropriate conditions to give ethanol. The reaction is

$$\mathrm{C}_2 \mathrm{H}_4(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(g) \rightleftharpoons \mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}(g)$$

An equilibrium mixture of these gases at a certain temperature had the following partial pressures: $P_{\mathrm{C}_2 \mathrm{H}_4}=0.575 \mathrm{~atm}$, $P_{\mathrm{H}_2 \mathrm{O}}=1.30 \mathrm{~atm}, P_{\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}}=6.99 \mathrm{~atm}$. What is the value of $K_{\mathrm{P}}$ ?