A student collected a 40.0 mL sample of H_{2} 2 gas at a temperature of 20.0°C and pressure of 720.0 mmHg. The next day the te
1 answer:
Answer: 750 mmHg
Explanation:
To calculate the new pressure, we use the equation given by Boyle's law. This law states that pressure is inversely proportional to the volume of the gas at constant temperature.
The equation given by this law is:
where,
= initial pressure of gas= 720.0 mmHg
= initial volume of gas = 40.0 ml
= final pressure of gas= ?
= final volume of gas = 38.4 ml
Putting values in above equation, we get:
Thus the new pressure will be 750 mmHg
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126 grams of H2O is formed.
Explanation:
Data given:
volume of the gas = 88 Liters
pressure = 720 mm Hg or 0.947 atm
temperature T = 22 Degrees or 295.15 K
R = 0.08021 atm L/mole K
n =?
The formula is used is of ideal gas law to know the number of moles of CH4 undergoing combustion.
PV = nRT
n =
putting the values in the equation
= 0.947 X 88/ 0.08021 X 295.15
n = 3.5 moles
balanced reaction for combustion of methane
CH4 + O2 ⇒ CO2 + 2H20
1 mole of CH4 undergoes combustion to form 2 moles of water
3.5 moles will give x moles of water
2/1 = x/3.5
x = 7 moles of water (atomic mass of water = 18 gram/mole)
mass = atomic mass x number of moles
mass = 18 x 7
=126 grams of water is formed.