The answer to your problem is 0.015 liters. I got the answer because to convert cubic centimeters into liters, you need to divide the cubic centimeters by 1000.
<u>Answer:</u> The final volume of the oxygen gas is 4.04 L
<u>Explanation:</u>
To calculate the final temperature of the system, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure and number of moles.
Mathematically,

where,
are the initial volume and temperature of the gas.
are the final volume and temperature of the gas.
We are given:

Putting values in above equation, we get:

Hence, the final volume of the oxygen gas is 4.04 L
<u>Answer:</u> The equilibrium concentration of CO is 0.243 atm
<u>Explanation:</u>
We are given:
Initial partial pressure of carbon dioxide = 0.902 atm
As, carbon dioxide is present initially. This means that the reaction is proceeding backwards.
For the given chemical equation:

<u>Initial:</u> 0.902
<u>At eqllm:</u> 3x (0.902-3x)
The expression of
for above equation follows:

We are given:

Putting values in above equation, we get:

So, equilibrium concentration of CO = 3x = (3 × 0.0810) = 0.243atm[/tex]
Hence, the equilibrium concentration of CO is 0.243 atm
Answer:
4.3043x10^24
Explanation:
Atoms(H) = (3.575 mol H2S/1)(2 mol H/1mol H2S)(6.02x10^23/1molH)
Simple stoicheometry problem. Sorry for taking so long, took Chem sophomore year, its been a while