What is the total pressure in a 6.00-L flask which contains 0.127 mol of H₂(g)and 0.288 mol of N₂(g)at 20.0°C? A)0)510 atm B)0)681 atm C)1)16 atm D)1)66 atm

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To solve this problem, we need to use the ideal gas law: PV = nRT where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. First, we need to calculate the total number of moles of gas in the flask: n(total) = n(H₂) + n(N₂) n(total) = 0.127 mol + 0.288 mol n(total) = 0.415 mol Next, we need to convert the volume of the flask to liters (it's given in milliliters): V = 6.00 L We also need to convert the temperature to Kelvin (add 273.15 to the Celsius temperature): T = 20.0°C + 273.15 T = 293.15 K Now we can plug in the numbers and solve for P: P = nRT/V P = (0.415 mol)(0.0821 L·atm/mol·K)(293.15 K)/(6.00 L) P = 1.66 atm Therefore, the answer is D) 1.66 atm.

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