Please answer the (a)

The insulating and packing material Styrofoam is a dating and packing material Styrofoam is a polymer of styrene. Find the molec

Nataly [62]

Explanation:

In order to find the molecular formula, we have to find the empirical formula first of all.

It is known that is a styrofoam, elements present are carbon and hydrogen atoms.

Element % Atomic mass Molar ratio Simple ratio

C 92.25 12.01 $\frac{92.25}{12.01}$ = 7.68 $\frac{7.68}{7.68}$ = 1

H 7.75 1.008 $\frac{7.75}{1.008}$ = 7.68 $\frac{7.68}{7.68}$ = 1

As empirical formula of styrofoam is C_{x}H_{x}.

Hence, empirical mass = (12.01 + 1.008) g/mol = 13.018 g/mol = 13.0 g/mol (approx)

Molar mass given is 104 g/mol.

So, $\frac{\text{molar mass}}{\text{empirical formula mass}}$ = $\frac{104}{13.0}$ = 8

Thus, we can conclude that molecular formula of the given styrene is $C_{8}H_{8}$ .

8 0

4 years ago

Look at the reaction below. Upper H subscript 2 upper S upper O subscript 4 (a q) plus upper Upper M g (s) right arrow Uper M g

Maslowich

Answer: D

H_2SO_4(aq)

Explanation:

Took it on edg and got it correct.

4 0

3 years ago

Read 2 more answers

At what temperature does sulfur tetrafluoride have a density of 0.230 g/L at 0.0721 atm?

Allisa [31]

Explanation:

At 365 K temperature sulfur tetrafluoride have a density of 0.260 g/L at 0.0721 atm.

What is an ideal gas equation?

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

First, calculate the moles of the gas using the gas law,

PV=nRT, where n is the moles and R is the gas constant. Then divide

the given mass by the number of moles to get molar mass.

Given data:

P= 0.0721 atm

n=\frac{mass}{molar \;mass}n=

molarmass

mass

R= 0.082057338 \;L \;atm \;K^{-1}mol^{-1}R=0.082057338LatmK

−1

mol

−1

T=?

Putting value in the given equation:

\frac{PV}{RT}=n

RT

PV

=n

density = \frac{2 \;atm\; X molar\; mass}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X T}density=

0.082057338LatmK

−1

mol

−1

XT

2atmXmolarmass

0.260 g/L = \frac{0.0721 \;atm\; X 108.07 g/mol}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X T}0.260g/L=

0.082057338LatmK

−1

mol

−1

XT

0.0721atmX108.07g/mol

T = 365.2158727 K= 365 K

Hence , at 365 K temperature sulfur tetrafluoride have a density of 0.260 g/L at 0.0721 atm.

8 0

1 year ago

Explain how the information given below could be used to determine the concentration of an unknown sample.

Vika [28.1K]

Answer:

See below

Explanation:Plot the known concentrations and adsorbance data. Draw a best fit line through thwe points. When the absorbance of a solution of unknown concentration (but same substance) is determined, find the concentration from the line at that absorption value. See attached graph.

E.g., an sample of the same substance had an absorbance of 0.35. Find that on the x scale and then determine the concentration that would be required to produce that level of absorbance. 0.483M in this case.