All categories

3 years ago

A 1300 mL sample of gas with a molar mass of 71.0 g/mol at STP has what density?

Chemistry

1 answer:

Blizzard [7]3 years ago

6 0

Answer:

0.055g/mL

Explanation:

Data obtained from the question include:

Molar Mass of the gass sample = 71g/mol

Volume of the gas sample = 1300 mL

Density =?

The density of a substance is simply mass per unit volume. It is represented mathematically as:

Density = Mass /volume.

With the above equation, we can easily obtain the density of sample of gas as illustrated below:

Density = 71g / 1300 mL

Density = 0.055g/mL

Therefore, the density of the gas sample is 0.055g/mL

You might be interested in

HELP!!!! A glass flask containing 100 milliliters of water is sealed with a rubber stopper and placed on a burner. After a while

kondor19780726 [428]

Answer: A closed system, because energy can enter or leave the container, but the water molecules cannot

Explanation:

Open system: In this system energy and matter both have access to their surroundings beyond the boundaries of system. .

Closed system :In this type system only energy has an access to its surroundings beyond the boundaries of system but not matter.

Isolated system:In this type system exchange of both energy and matter are restricted to move outside the boundaries of system.

According to question, the system given is a closed system because energy is transferred from the burner to glass flask and from the glass flask to the water (matter). But water molecules are only getting condensed on the inside surface of the flask that is exchange of matter beyond the boundaries of the system is restricted. Hence, closed system ,A closed system, because energy can enter or leave the container, but the water molecules cannot.

7 0

3 years ago

We bored Meeting id:333-065-2087 Password:5FRgXJ

Juli2301 [7.4K]

Answer:

pls don't post irrelevant questions

Explanation:

FOLLOW MY ACCOUNT PLS PLS

4 0

3 years ago

Read 2 more answers

At elevated temperature, carbon tetrachloride decomposes to its elements: CCl4(g) C(s) 2Cl2(g). At 700 K, if the initial pressur

PIT_PIT [208]

Answer:

$K=0.0131M$

Explanation:

Hello,

In this case, the undergoing chemical reaction turns out:

$CCl_4(g) \rightleftharpoons C(s)+ 2Cl_2(g)$

In such a way, by means of the mass of law action for such reaction, which is given below:

$Kp=\frac{p_{Cl_2}^2}{p_{CCl_4}}$

And in terms of the change $x$ due to reaction extent:

$p_{CCl_4}=p_{CCl_4}^0-x\\p_{Cl_2}=2x\\p_T=p_{CCl_4}+p_{Cl_2}=1.00-x+2x\\p_T=1.00+x$

$x$ results:

$x=1.35 atm -1.00atm=0.35atm$

In such a way, Kp:

$Kp=\frac{(2x)^2}{1.00-x} =\frac{(2*0.35atm)^2}{1.00atm-0.35atm}=0.754atm$

Nonetheless, K is asked instead of Kp, thus:

$K=\frac{Kp}{(RT)^{\Delta \nu _{gas}}}$

Whereas:

$\Delta \nu _{gas}=2-1=1$

Which is the change in the moles of gaseous species chlorine and carbon tetrachloride. Hence, we finally obtain:

$K=\frac{0.754atm}{(0.082\frac{atm*L}{mol*K}*700K)^{1}}\\\\K=0.0131mol/L=0.0131M$

Best regards.

8 0

3 years ago

2.54 mL of ethanol to mol ethanol (Hint: the density of ethanol is 0.789 g/mL.)

Katarina [22]

0.04350179862

Explanation:

Make sure to check for sig figs though. Basically, you have 2.54 mL and you multiply that by the 0.789 g/mL and mL cancels out and you are left with 2.00406g. There are 46.06844 grams per mol of ethanol, so to cancel out grams we multiply by 1/46.06844. And then we are left with 0.04350179862 mol

7 0

4 years ago

)- symbols following elements silver, Copper ,magnesium ,sulphur

NNADVOKAT [17]

Ag,Cu,Mg,S are the answers...............

3 0

3 years ago

Read 2 more answers