how do you solve for the combined gas law?..i ..I am very confused ..someone help by making it easier and clear since i am kinda slow..
ex.a sample of neon gas has a volume of 752ml at 25.0C. what will the volume at 50.0C be if pressure is constant
ahh i hate chemisty, i'm kindof slow too and everything confuses me in chem.!! i feel the same way as you:)
I just remember the combined gas law as one law; i.e.,
(P1V1)/T1= (P2V2)/T2
Since P is constant, just cover P1 and P2 and you are left with the expression of
V1/T1 = V2/T2
V1 = 752 mL
T1 = 25 C = 273 + 25 = 298 K
V2 = ??
T2 = 50 + 273 = 323 K
So
752/298 = V2/323
Cross multiply
298*V2 = 752*323
solve for V2
V2 = (752*323)/298 = 815.087 mL which rounds to 815 mL.
There is no reason to be confused. Just remember to use logic to think your way through problems.
thanxs sooo much i understand now, all i need is practice
To solve for the combined gas law, you can use the formula:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
where P represents pressure, V represents volume, and T represents temperature.
In your specific example, the pressure is constant, so we can simplify the formula to:
(V1 / T1) = (V2 / T2)
Now let's plug in the given values:
V1 = 752 mL
T1 = 25.0 °C = 25.0 + 273.15 = 298.15 K
T2 = 50.0 °C = 50.0 + 273.15 = 323.15 K
Now we can solve for V2:
(V1 / T1) = (V2 / T2)
(752 mL / 298.15 K) = (V2 / 323.15 K)
Now we cross-multiply and solve for V2:
752 mL * 323.15 K = 298.15 K * V2
V2 = (752 mL * 323.15 K) / 298.15 K
V2 ≈ 815 mL
Therefore, the volume of the neon gas at 50.0 °C would be approximately 815 mL, assuming the pressure remains constant.