Answer
To find the volume occupied by 1.00 mol of air under the given conditions, we can use the ideal gas law:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature.
First, we need to convert the temperature from Celsius to Kelvin:
T = -19°C + 273.15 = 254.15 K
Next, we can use the ideal gas law to solve for the volume:
V = nRT / P
We know that n = 1.00 mol, R = 8.31 J/(mol·K), P = 33.7 kPa, and T = 254.15 K. Substituting these values, we get:
V = (1.00 mol) (8.31 J/(mol·K)) (254.15 K) / (33.7 kPa) = 0.202 m^3
Therefore, the volume occupied by 1.00 mol of air at the summit of Everest is 0.202 $m^3$.
Work Step by Step
To find the volume occupied by 1.00 mol of air under the given conditions, we can use the ideal gas law:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature.
First, we need to convert the temperature from Celsius to Kelvin:
T = -19°C + 273.15 = 254.15 K
Next, we can use the ideal gas law to solve for the volume:
V = nRT / P
We know that n = 1.00 mol, R = 8.31 J/(mol·K), P = 33.7 kPa, and T = 254.15 K. Substituting these values, we get:
V = (1.00 mol) (8.31 J/(mol·K)) (254.15 K) / (33.7 kPa) = 0.202 m^3
Therefore, the volume occupied by 1.00 mol of air at the summit of Everest is 0.202 $m^3.$
