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i need help with soem chem homework ?
A container of argon has a pressure of 720 torr and a volume of 256 mL at 25.0°C. What is the pressure of
the argon if the volume changes to 2.23 L and the temperature increases to 50.0°C?
1 Answer
- xener70Lv 42 weeks ago
In order to ease calculations, we can suppose Argon as ideal gas. Then we might use ideal gasses equation P*V=n*R*T. Nothing indicates that amount of argon changes, only its conditions varies. So, we certainly know that value for n is constant, also R is always constant, meaning that
P1 * V1 = n*R * T1 and P2 * V2 = n*R * T2. Now that you can use constant (n*R) = (P1*V1 / T1) = (P2*V2 / T2)
Resolving ----- P1*V1*T2 = P2*V2*T1.
The problem is asking for the value of P2,
P2 = (P1*V1*T2) / (V2*T1)
Excellent tip_ At the momment you have a mix of Units for the all the gas conditions, the best thing is to convert them within a single system of units, you can choose International System (atm, l, K, etc) for example. It is PRIORITY TO USE TEMPERATURE VALUES IN KELVIN.
P1 = 720 torr = (720/760) atm = 0.94736842 atm
V1 = 256 ml = 0.256 l
T1 = 25.0 C = (273.12 + 25) K = 298.12 K
V2 = 2.23 l
T2 = 50.0 C = (273.12 + 50) K = 223.12 K
