Answer:
There are 1.287 grams of acetylene collected
Explanation:
Total gas pressure = 909 mmHg
Vapor pressure of water = 20.7 mmHg
Pressure of acetylene = 909 mmHg - 20.7 mmHg = 888.3 mmHg
1mmHg = 1 torr
22 ° C + 273.15 = 295.15 Kelvin
Ideal gas law ⇒ pV = nRT
⇒ with p = pressure of the gas in atm
⇒ with V = volume of the gas in L
⇒ with n = amount of substance of gas ( in moles)
⇒ with R = gas constant, equal to the product of the Boltzmann constant and the Avogadro constant (62.36 L * Torr *K^−1 *mol^−1)
⇒ with T = absolute temperature of the gas (in Kelvin)
888.3 torr * 1.024 L = n * 62.36 L * Torr *K^−1 *mol^−1 * 295.15 K
n = 0.04942 moles of C2H2
Mass of C2H2 = 0.04942 moles x 26.04 g/mole = 1.287 g
There are 1.287 grams of acetylene collected
