There is a balloon filled with methane,CH4. If the mass of the methane is 68.34g, what is the volume of the balloon at 0.805 atm and a temperature of -10*C?
PV=nRT
V= nRT/P n = moles= mass/molmassCH4
change temp in C to K
so what is the molar mass? i know that v= ? * .805/263K, but im stuck on this one???
Can't you calculate the molar mass of CH4. Look on the periodic table. Atomic mass C + 4*atomic mass H = molar mass CH4.
To solve this problem, we can use the ideal gas law, which states that 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 the temperature from Celsius to Kelvin. We add 273 to the Celsius temperature to get:
T = (0°C + 273) K
T = 273 K
Next, we need to calculate the number of moles of methane (CH4). To do this, we can use the formula:
moles = mass / molar mass
The molar mass of methane (CH4) is 16 g/mol (12 g/mol for carbon + 4 g/mol for hydrogen). Plug in the values:
moles = 68.34 g / 16 g/mol
moles = 4.27 mol
Now we can substitute the values into the ideal gas law equation:
PV = nRT
V = (nRT) / P
V = (4.27 mol × 0.0805 L·atm/(mol·K) × 273 K) / 0.805 atm
Simplifying the equation, we find:
V = 94.77 L
Therefore, the volume of the balloon filled with methane at 0.805 atm and a temperature of -10°C is approximately 94.77 liters.