Answer :
Answer:
P = 24.34 atm
Explanation:
V = 5.0L
P = ?
n = 4.75 moles
T = 39.3°C = (39.3 + 273.15)K = 312.45K
From ideal gas equation,
PV = nRT
P = pressure of the gas
V = volume of the gas
n = no. Of moles present
R = ideal gas constant = 0.082atm.L / mol.K
PV = nRT
P = nRT / V
P = (4.75 * 0.082 * 312.45) / 5
P = 121.699 / 5
P = 24.339 atm
P = 24.34 atm
The pressure of the gas is 24.34 atm
Final answer:
The pressure in a 5.00 L tank with 4.75 moles of oxygen at 39.3 °C is calculated using the ideal gas law, resulting in approximately 24.65 atm.
Explanation:
To calculate the pressure of a gas in a tank, we can use the ideal gas law which is 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, convert the temperature from degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature:
T = 39.3 °C + 273.15 = 312.45 K
Next, use the ideal gas law to calculate the pressure:
P =[tex]\frac{nRT}{V}[/tex]
Given n = 4.75 moles, T = 312.45 K, V = 5.00 L, and R = 0.0821 atm·L/mol·K (value of the ideal gas constant when pressure is measured in atmospheres), we can calculate the pressure:
P = [tex]\frac{(4.75 moles)(0.0821 atm·L/mol·K)(312.45 K)}{5.00 L}[/tex]
Doing the calculation:
P =[tex]\frac{(4.75)(0.0821)(312.45)}{5.00}[/tex] = 24.65 atm
This means the pressure inside the 5.00 L tank containing 4.75 moles of oxygen at 39.3 °C is approximately 24.65 atmospheres.
