180g of zinc metal was dropped into a beaker of hydrochloric acid, After the reaction stopped,
35 grams of reacted zinc remained. Calculate;- Mass or HCI that reacted.
ii) Volume of H2) produced.
To calculate the mass of hydrochloric acid (HCI) that reacted, we need to find the difference between the initial mass of zinc and the remaining mass of reacted zinc.
Initially, there were 180g of zinc metal.
After the reaction, 35g of zinc remained.
Mass of HCI that reacted = Initial mass of zinc - Mass of reacted zinc
Mass of HCI that reacted = 180g - 35g = 145g
Therefore, 145 grams of hydrochloric acid reacted.
To calculate the volume of H2 gas produced, we need to use the stoichiometry of the balanced chemical equation. The balanced equation for the reaction between zinc and hydrochloric acid is:
Zn + 2HCl -> ZnCl2 + H2
The coefficient in front of H2 is 1, which means for every 1 mole of zinc that reacts, 1 mole of H2 gas is produced.
To find the volume of H2 gas produced, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (assume atmospheric pressure if not specified)
V = volume of gas
n = number of moles of gas
R = ideal gas constant (0.0821 L*atm/mol*K)
T = temperature (usually in Kelvin)
First, calculate the number of moles of H2 gas produced:
Number of moles of H2 = Number of moles of reacted zinc (assume complete reaction)
Number of moles of reacted zinc = mass / molar mass of zinc
Number of moles of reacted zinc = 35g / 65.38 g/mol (molar mass of zinc)
Now, we can use the ideal gas law equation to calculate the volume of H2 gas:
PV = nRT
Assuming atmospheric pressure (1 atm) and room temperature (298 K), we have:
(1 atm)(V) = (Number of moles of H2 gas)(0.0821 L*atm/mol*K)(298 K)
V = (Number of moles of H2 gas)(0.0821 L*atm/mol*K)(298 K)
Now, substitute the value of the number of moles of H2 gas:
V = (35g / 65.38 g/mol)(0.0821 L*atm/mol*K)(298 K)
Calculating this expression will give you the volume of H2 gas produced in liters.