A balloon of methane gas, CH4, has a temperature of -2 degrees celcius and contains 2.35g of the gas. What is the temperature in kelvin and how many moles of gas does the balloon contain?
first figure the moles from the mass.
Kelvin= 273-2
To find the temperature in Kelvin, you need to use the Kelvin scale, which is an absolute temperature scale where 0 K represents absolute zero. The formula to convert from Celsius to Kelvin is:
T(K) = T(°C) + 273.15
So, to convert -2 °C to Kelvin:
T(K) = -2 + 273.15 = 271.15 K
To calculate the number of moles of gas in the balloon, you can use the ideal gas law. The ideal gas law equation is:
PV = nRT
Where:
P is the pressure of the gas,
V is the volume of the gas,
n is the number of moles of gas,
R is the ideal gas constant (0.0821 L·atm/(mol·K)),
T is the temperature in Kelvin.
Since the question doesn't provide the pressure or volume of the gas, we can assume they are constant. Therefore, we can rewrite the ideal gas law equation as:
n = (PV) / (RT)
Now we can calculate the number of moles of gas:
n = (PV) / (RT) = (PV) / (0.0821 * T)
To calculate the number of moles of gas, we need to know the pressure and volume of the balloon. If these values are not provided, we cannot accurately calculate the number of moles.