This problem. We're going to do a series of calculation using the ideal gas law PV equals NRT. If we're going to use our equal 2.08-1 that's in leader atmospheres per mole Calvin. So we're going to need to make sure that we have volume and leaders pressure and atmospheres and we'll have moles and our temperature of course will be in kelvin. Mhm. So for this 1st 1 so we've got P. D. Equals NRT. So we're giving a pressure of 1.77 ATM And we've got 4.98 l and we're looking for moles because we don't have that Put away to one And our temperature is 43.1°C.. So add to 73 .15 to that. So then we'll go ahead and solve for moles and we're gonna come out with 0.339 moles. So we can fill that into the table. And then we're gonna multiply by the molar mass of, We're using N 204. So it's going to be 92.02 g per mole. So if we multiply there we'll get 31 .2 g and can fill in that into the table as well. So on the second one, we've got our pressure and volume and some moles. Okay, so again, T. V. Equals NRT. So our pressure is 673 But it's mm of Mercury. So I'm gonna need to divide by 760 to go ahead and get that into atmospheres. Okay. Um are Volume is 488 ml. But we need that to be in leaders. So .488 leaders. Mhm. And we've got malls, So .783 moles .08- one. And one of the things we're missing here is temperature. So we'll go ahead and solve for temperature. We're going to get 6.72 Kelvin. And the other thing that we're missing here is grams. So we're gonna go ahead and take our moles, which is point 783 moles. Again, we're gonna go ahead and multiply that by our molar mass, 92 oh two g per mole. And that will give us 72 0.1 g. So those are the missing pieces of the table for part B. So in part C, we've got our pressure. Okay, They've given it to us in bar. So let's go ahead and make some conversions here, .899 Bar, If we multiply that by 100 we'll get killer Pascal's. So we've got 89.9 kpa. And then why don't we go ahead and change that atmosphere so we can plug it into our um ideal gas law, Which is one on 1 0.3. So this is going to come out to be point eight 87 ATM They've given us the mass which is 6.25 g. And we're gonna need to go ahead and change that to moles 92.02. So if we do that, we've got .0679 moles. So that's one of the things missing in the table. So we'll go ahead and circle that and our temperature is 912 degrees Celsius. So let's go ahead and change that to kelvin. So we'll get 1185 kelvin and then we can go ahead and calculate are missing volume. So PV equals NRT. We had plug in the things. We just found some 887 ATM mhm. And our volume here actually, the volume is what we're missing. Right? So we're gonna go ahead and calculate that volume And our moles is .0679 And .08- one. And our temperature 1185. So if we do out our math and we saw for our volume will get 7.45 l plug that into our table. Okay, so our last example here, we've got a volume and a temperature in Fahrenheit and some moles. So first thing, why don't we go ahead and get that Fahrenheit temperature into Celsius and then kelvin, So degrees Celsius is 5/9 of Fahrenheit, so are 39 F -32. That's how you convert from Fahrenheit to C. So we're going to get 3.88 degrees Celsius, We'll go ahead and add to 73 .15 to convert that to Calvin to 77.4 Kelvin and then plugging into piven ERT vehicles and artie uh huh We're looking for a pressure mm Oops, And we've got a volume which is 1.15 L. Mhm and we've got .166 moles was given .08- one. And that temperature we just found 277 point oh four. So calculate our pressure. We come out with 3-8 ATM there's a missing piece of our table and the last missing piece was our graham. So we're just gonna go ahead and change our malls again by multiplying by our molar mass you grams per more. And that will give us 15 0.3 g. So now we've identified all the missing pieces of the table.