<span>Sb2O3 + SbCl3 = Sb4O5Cl2
To balance Cl each side from Cl3 and Cl2 .. need 6 Cl
Sb2O3 + 2SbCl3 = 3Sb4O5Cl2
now to balance O.... O3 and O5 ... so need 15O
5Sb2O3 + 2SbCl3 = 3Sb4O5Cl2
Now check Sb each side 10 + 2 = 3x4 = 12 so OK</span>
This problem is describing the state two gases have when separated and together as shown on the attached picture. First of all, diagram 1 shows how they are separated in two containers with apparently equal volumes, whereas diagram 2 shows the removal of the barrier so that they get mixed together.
In this case, we can analyze that each gas has its own pressure and due to the removal of the barrier, both pressure and volume undergo a change. Thus, we can infer that the final volume is doubled with respected to the initial one for each gas, causing the pressure of each gas to be halved and the total pressure the half of the added ones, in agreement to the Boyle's law (inversely proportional relationship between pressure and temperature).
Therefore, the correct choice is:
C. The partial pressure of each gas in the mixture is half its initial pressure; the final total pressure is half the sum of the initial pressures of the two gases.
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We are given the chemical reaction and the amount of fuel used for the process. We use these data together with the molar masses to obtain what is asked. We do as as follows:
100 g C8H18 ( 1 / 114.33) ( 16 / 2 ) = 6.9973 mol CO2 produced
hydrogen react with oxygen to form water as per the equation below
2H2 + O2 =2H2O
This reaction can be described in words as follows
two molecules of hydrogen react with one molecule of oxygen to form two molecules of water.