Answer:A
Explanation:I hope I’m right
Atoms are the basic building blocks of ordinary matter. Atoms can join together to form molecules, which in turn form most of the objects around you.
Answer:
The partial pressure of oxygen in the mixture is 296 mmHg.
Explanation:
The pressure exerted by a particular gas in a mixture is known as its partial pressure. So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone.
This relationship is due to the assumption that there are no attractive forces between the gases.
So, in this case, the total pressure is:
PT=Phelium + Pnitrogen + Poxygen
You know:
- PT= 756 mmHg
- Phelium= 122 mmHg
- Pnitrogen= 338 mmHg
- Poxygen= ?
Replacing:
756 mmHg= 122 mmHg + 338 mmHg + Poxygen
Solving:
756 mmHg - 122 mmHg - 338 mmHg = Poxygen
Poxygen= 296 mmHg
<u><em>The partial pressure of oxygen in the mixture is 296 mmHg.</em></u>
12.5% of strontium-90 would remain in a sample after three half-lives have passed. Half-life automatically means 50% of the original amount would remain.
Answer:
The partial pressure in mm Hg for each of the species are:
PCO = 0
PH2 = 3874
PCH3OH = 347
The total pressure is 4221
Explanation:
We have to use Ideal gas equation PV = nRT and Partial pressure rule Total Pressure= ∑ Partial pressures.
We have following data:
T= 357K (85+272); nCO=0.078 (2.2/28); nH2 = 2.43 (4.86/2); R=62.36
With equation CO(g) + 2 H2(g) → CH3OH(g) we can calculate the amount of moles the reaction has finished. The limit reagent is CO because is consumed completely and moles CO in flask are 0. According to equation, every CO mol produces one CH3OH mol. That means 0.078 CO moles produces 0.078 CH3OH moles. From Ideal gas equation we have P=nRT/V.
Applying:
PH2=0.87*62.36*357/5=3874
PCH3OH =0.078*62.36*357/5=347
Total P = 3874+347=4221
I hope my answer helps you
