00:01
Hi, so to solve for this, let us calculate first the number of moles of oxygen gas using the ideal gas equation pv is equivalent to nrt.
00:14
So rearranging this to solve for the number of moles, o2 will have pv over rt.
00:22
So the pressure is said to be, this is at stp so that means, let's write here at stp the temperature will be equivalent to 273 kelvin or 0 .15, 273 .15 kelvin or you can just write 273 and then the pressure is 180 m.
00:42
Okay, so these are the values of the temperature and pressure at standard temperature and pressure or stp.
00:48
So we'll write here 180 m.
00:51
The volume is 35 liters.
00:53
R is the gas constant, 0 .0821 liters, 80 m per mole kelvin and then the temperature we have 273 kelvin.
01:05
So now we'll cancel some units, we'll cancel liters and 80 m and then the kelvin and the remaining unit as you can see is moles.
01:13
So we'll have 0 .12817, this is moles of oxygen gas.
01:20
Now we will calculate the number of moles of chlorine gas required to react to the given amount of o2.
01:31
So if we have 0 .12817, this is moles of o2.
01:36
As per your balance equation, 7 moles of o2 will react with 2 moles of cl2 and then we cancel moles of o2 here, we'll get 0 .03662...