A piece of Pyramid museum was reacted with excess athletes hydrochloric acid in 166 himalaya gas with pressure of 0.995 ATM was collected by water displacement method at 36°C the vapor pressure water is 44.6 tour how many moles of H2 gas were produced
To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas (in atm)
V = volume of the gas (in liters)
n = number of moles of gas
R = gas constant (0.08206 L.atm/mol.K)
T = temperature of the gas (in Kelvin)
First, let's calculate the volume of the gas produced using the water displacement method. Since the pressure of the gas collected is 0.995 atm and the pressure of water vapor is 44.6 torr, we need to convert the water vapor pressure to atm:
44.6 torr / 760 torr/atm = 0.0588 atm
Therefore, the total pressure of the gas collected is:
0.995 atm + 0.0588 atm = 1.0538 atm
Next, plug in the values:
PV = nRT
1.0538 atm * V = n * 0.08206 L.atm/mol.K * 309 K
V = n * 0.08206 * 309 / 1.0538
V = 24.08n
Now, we need to convert the volume to moles of H2 gas using the ideal gas law:
PV = nRT
1.0538 atm * 24.08n = n * 0.08206 L.atm/mol.K * 309 K
n = (1.0538 * 24.08) / (0.08206 * 309)
n ≈ 0.298 moles
Therefore, approximately 0.298 moles of H2 gas were produced.