When 1.53 grams of silver metal are dropped in 500. mL of 2.0 M acetic acid, how many liters of gas are evolved at STP?
To determine the number of liters of gas evolved at STP, we need to start by balancing the chemical equation for the reaction of silver metal (Ag) with acetic acid (CH3COOH). The balanced equation is as follows:
2Ag + 2CH3COOH -> 2CH3COOAg + H2(g)
From the balanced equation, we can see that 2 moles of silver (Ag) react with 2 moles of acetic acid (CH3COOH) to produce 2 moles of silver acetate (CH3COOAg) and 1 mole of hydrogen gas (H2).
Next, we need to determine the number of moles of silver (Ag) present in 1.53 grams. The molar mass of silver is 107.87 g/mol. Therefore, the number of moles of silver can be calculated as follows:
Moles of Ag = Mass of Ag / Molar mass of Ag
= 1.53 g / 107.87 g/mol
≈ 0.0142 mol
Since the stoichiometry of the balanced chemical equation tells us that 2 moles of silver (Ag) react to produce 1 mole of hydrogen gas (H2), we can determine the number of moles of hydrogen gas that will be evolved:
Moles of H2 = 0.0142 mol / 2
= 0.0071 mol
Now, we can use the ideal gas law to convert the number of moles of hydrogen gas to liters at STP (standard temperature and pressure). According to the ideal gas law, the molar volume of an ideal gas at STP is 22.4 liters/mol. Therefore, the number of liters of hydrogen gas at STP can be calculated as follows:
Liters of H2 = Moles of H2 * Molar volume at STP
= 0.0071 mol * 22.4 L/mol
= 0.16 L
Therefore, approximately 0.16 liters of gas will be evolved at STP when 1.53 grams of silver metal are dropped in 500 mL of 2.0 M acetic acid.