Question

A cylinder contains 11.8L of air at a total pressure of 43.2 psi and a temperature of 25°C. How many moles of gas does the cylinder contain?(Hint: you must convert each quantity into the correct units (L,ATM,mol,and K) before substituting into the ideal gas law.)

Answer 1

To find the number of moles of gas in the cylinder, we can use the ideal gas law equation PV = nRT. After converting the temperature from Celsius to Kelvin and the pressure from psi to atm, we can substitute the values into the equation and solve for n. The cylinder contains 0.57 moles of gas.

Step-by-step explanation:

To solve this problem, we need to 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 by adding 273.15: 25°C + 273.15 = 298.15K.

Next, we need to convert the pressure from psi to atm by dividing by 14.7: 43.2 psi / 14.7 psi/atm = 2.94 atm.

The given volume is already in liters, so we don't need to make any changes. Now we can substitute the values into the ideal gas law equation and solve for n:

n = PV / RT = (2.94 atm) * (11.8 L) / [(0.0821 L*atm/mol*K) * 298.15K]

= 0.57 moles

Therefore, the cylinder contains 0.57 moles of gas.