How many moles of helium gas are contained in a 43.0 L flask at STP?A.0.089 molB.89 molC.0.045 molD.0.17 mol

To solve this problem, we need to use the ideal gas law, which states that the volume of a gas is directly proportional to the number of moles of the gas and the temperature, and inversely proportional to the pressure. At standard temperature and pressure (STP), one mole of any gas will occupy 22.4 liters.

Step 1: Identify the given volume and the volume of one mole of gas at STP. The given volume is 43.0 L and the volume of one mole of gas at STP is 22.4 L/mol.

Step 2: Use the formula for the ideal gas law at STP, which is V = n * Vm, where V is the volume of the gas, n is the number of moles of the gas, and Vm is the molar volume of the gas at STP.

Step 3: Rearrange the formula to solve for n, the number of moles. The rearranged formula is n = V / Vm.

Step 4: Substitute the given values into the formula. n = 43.0 L / 22.4 L/mol = 1.92 mol.

So, none of the options A, B, C, or D is correct. The number of moles of helium gas in a 43.0 L flask at STP is approximately 1.92 mol.