A sample of H2 gas occupies a volume of 565 mL at STP. What, volume, in mL, will this sample of H2gas occupy at a temperature of -17oC and at a pressure of 0.560 atm
Do you know that STP stands for standard temperature and pressure.
Standard T is 273 K and standard pressure is 1 atmosphere.
Use (P1V2/T1) = (P2V2/T2)
Don't forget to change degrees C to kelvin. Post your work if you run into trouble.
946mL
Correct. Good work.
To solve this problem, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert -17°C to Kelvin by adding 273.15 to the temperature:
T = -17°C + 273.15 = 256.15 K
At STP (Standard Temperature and Pressure), the pressure is 1 atmosphere (atm), and the temperature is 0°C or 273.15 K.
We can solve for n (the number of moles) at STP using the ideal gas law equation:
PV = nRT
(1 atm)(565 mL) = n(0.0821 L·atm/mol·K)(273.15 K)
565 mL is equal to 0.565 L.
Solving for n:
n = (1 atm * 0.565 L) / (0.0821 L·atm/mol·K * 273.15 K)
n ≈ 0.024 moles
Now, we can use the same equation to find the volume at the new temperature and pressure:
(0.560 atm)(V) = (0.024 moles)(0.0821 L·atm/mol·K)(256.15 K)
Solving for V:
V = (0.024 moles)(0.0821 L·atm/mol·K)(256.15 K) / (0.560 atm)
V ≈ 2.02 L
Finally, we need to convert this volume from liters to milliliters:
V ≈ 2.02 L * 1000 mL/L
V ≈ 2020 mL
Therefore, the sample of H2 gas will occupy a volume of approximately 2020 mL at a temperature of -17°C and a pressure of 0.560 atm.