3. Fill in: Name the organelle or organelles that perform each of the following functions.

A 16 gram sample of O2(g) fills a container at STP. What volume is the container?

sergij07 [2.7K]

Answer:

V = 11.2 L

Explanation:

Hello there!

In this case, according to the ideal gas equation:

$PV=nRT$

It is possible to compute the volume as shown below:

$V=\frac{nRT}{P}$

Whereas the moles are computed are computed given the mass and molar mass of oxygen:

$n=16g*\frac{1mol}{32g} =0.5mol$

Now, since the STP stands for a temperature of 273.15 K and a pressure of 1 atm, the resulting volume is:

$V=\frac{0.5mol*0.08206\frac{atm*L}{mol*K}*273.15K}{1atm}\\\\V=11.2L$

Best regards!

8 0

2 years ago

What happens to the atomic mass of an element moving from left to right within a period

JulsSmile [24]

Answer:

As you move across a period, the atomic mass increases because the atomic number also increases. ... The atomic mass for any given atom mainly comes from the mass of the protons and neutrons.

Explanation:

4 0

3 years ago

Gaseous methane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 9.6 g of methane is

lianna [129]

Answer:

21.6 g

Explanation:

The reaction that takes place is:

CH₄ + 2O₂ → CO₂ + 2H₂O

First we convert the given masses of both reactants into moles, using their respective molar masses:

9.6 g CH₄ ÷ 16 g/mol = 0.6 mol CH₄

64.9 g O₂ ÷ 32 g/mol = 2.03 mol O₂

0.6 moles of CH₄ would react completely with (2 * 0.6) 1.2 moles of O₂. As there are more O₂ moles than required, O₂ is the reactant in excess and CH₄ is the limiting reactant.

Now we calculate how many moles of water are produced, using the number of moles of the limiting reactant:

0.6 mol CH₄ * $\frac{2molH_2O}{1molCH_4}$ = 1.2 mol H₂O

Finally we convert 1.2 moles of water into grams, using its molar mass:

1.2 mol * 18 g/mol = 21.6 g

4 0

2 years ago

What is the wavelength of light with 2.89 x 10-19 J of energy? (The speed of

Alika [10]

Let's see

$\\ \rm\rightarrowtail E=hv$

$\\ \rm\rightarrowtail E=\dfrac{hc}{\lambda}$

lambda is wavelength
h is Planck constant
c is velocity of sound in air
E in energy

$\\ \rm\rightarrowtail \lambda=\dfrac{hc}{E}$

$\\ \rm\rightarrowtail \lambda=\dfrac{6.626\times 10^{-34}\times 3\times 10^8}{2.89\times 10^{-19}}$

$\\ \rm\rightarrowtail \lambda=6.878\times 10^{-7}m$

$\\ \rm\rightarrowtail \lambda=68.8\mu m$

3 0

2 years ago

Calculate the number of moles of H2 produced in the reaction of Mg(s) with HCl(aq). Mg(s) is the

Taya2010 [7]

Explanation:

Moles of metal,

=

4.86

⋅

g

24.305

⋅

g

⋅

m

o

l

−

1

=

0.200

m

o

l

.

Moles of

H

C

l

=

100

⋅

c

m

−

3

×

2.00

⋅

m

o

l

⋅

d

m

−

3

=

0.200

m

o

l

Clearly, the acid is in deficiency ; i.e. it is the limiting reagent, because the equation above specifies that that 2 equiv of HCl are required for each equiv of metal.

So if

0.200

m

o

l

acid react, then (by the stoichiometry), 1/2 this quantity, i.e.

0.100

m

o

l

of dihydrogen will evolve.

So,

0.100

m

o

l

dihydrogen are evolved; this has a mass of

0.100

⋅

m

o

l

×

2.00

⋅

g

⋅

m

o

l

−

1

=

?

g

.

If 1 mol dihydrogen gas occupies

24.5

d

m

3

at room temperature and pressure, what will be the VOLUME of gas evolved?

5 0

2 years ago