A gas that occupies a volume of 6.75L at 89.0atm will occupy what volume at 68.55mm Hg if the temperature remains constant?
(89.0atm/0.09atm)*6.75=6,680
V2=6680
Is this right??
Close but no cigar.
I think you have made two errors. First, I think you punched the calculator wrong. If I punch in the numbers you show I don't get 6680 but 6675. Second, you dropped two digits on the 0.09 conversion. 68.55/760 = 0.0901974 which would round to 0.0902. When you work the problem piece meal like that you make rounding errors. Sometimes they are critical. What I do is leave the number in the calculator and just do a string of calculations.
But even rounding to 0.0902 gives 6660 liters. If your prof is a stickler for significant digits s/he will want you to write 6.66 x 10^3 liters and not 6660 liters.
No, your calculation is incorrect. To solve this problem, you can use Boyle's Law, which states that the volume of a gas is inversely proportional to the pressure, assuming constant temperature.
Boyle's Law equation:
P1 * V1 = P2 * V2
Given:
P1 = 89.0 atm
V1 = 6.75 L
P2 = 68.55 mm Hg
First, convert the pressure from mm Hg to atm:
1 atm = 760 mm Hg
P2 = 68.55 mm Hg / 760 mm Hg/atm = 0.09 atm
Now substitute the values into the equation:
89.0 atm * 6.75 L = 0.09 atm * V2
To solve for V2, divide both sides of the equation by 0.09 atm:
(89.0 atm * 6.75 L) / 0.09 atm = V2
V2 = 6.679 L (rounded to three significant figures)
So, the gas will occupy a volume of approximately 6.679 L at 68.55 mm Hg, assuming constant temperature.
To solve this problem, you need to use the combined gas law equation:
P1 * V1 / T1 = P2 * V2 / T2
Where:
P1 and P2 are the initial and final pressures, respectively
V1 and V2 are the initial and final volumes, respectively
T1 and T2 are the initial and final temperatures, respectively
In this case, the temperature remains constant, so T1 = T2. Also, we are given:
P1 = 89.0 atm
V1 = 6.75 L
P2 = 68.55 mm Hg
Now, we need to convert the pressure from mm Hg to atm:
68.55 mm Hg * (1 atm / 760 mm Hg) = 0.0901 atm
Substituting the values into the combined gas law equation:
(89.0 atm) * (6.75 L) / T1 = (0.0901 atm) * V2 / T1
Now, we can solve for V2:
(89.0 atm * 6.75 L) / (0.0901 atm) = V2
V2 ≈ 6653 L
Therefore, the gas will occupy approximately 6653 L at 68.55 mm Hg if the temperature remains constant.
So, in your calculation, you made a slight mistake with converting the pressure from mm Hg to atm. Instead of using 0.09 atm, you should have used the converted value of 0.0901 atm, which would give you the correct answer of V2 = 6653 L.