Final answer:
To find the number of moles of CO in a 5.00 L tank at 155°C and 2.80 atm, use the ideal gas law equation, resulting in approximately 0.39 moles of CO.
Step-by-step explanation:
The question concerns how many moles of carbon monoxide (CO) are contained in a 5.00 L tank at 155°C and 2.80 atm. To solve this problem, we use the ideal gas law, which is represented by the formula PV = nRT, where P is pressure, V is volume, n is the number of moles of the gas, R is the ideal gas constant, and T is temperature in Kelvin.
Firstly, we need to convert the temperature from °C to Kelvin by adding 273.15, which gives us a temperature of 155 + 273.15 = 428.15 K. Then, using the ideal gas constant R = 0.08206 L·atm/mol·K, we can rearrange the ideal gas law to solve for n (the number of moles): n = PV / (RT). By substituting the values, we get n = (2.80 atm × 5.00 L) / (0.08206 L·atm/mol·K × 428.15 K).
Performing the calculation yields n = 0.39 moles of CO approximately.