If 3 L of hydrogen and 1.5 L of oxygen at STP react to yield water how many moles of water are formed? What gas volume does the water have at a temperature of 100degrees C and 1 atm pressure?
yass
To determine the moles of water formed when hydrogen and oxygen react, we need to consider the balanced chemical equation for the reaction:
2H₂ + O₂ → 2H₂O
From the equation, we can see that for every 2 moles of hydrogen, we produce 2 moles of water. Therefore, we need to convert the given volume of hydrogen to moles and then find the corresponding moles of water formed.
Given:
Volume of hydrogen (H₂) = 3 L
Volume of oxygen (O₂) = 1.5 L
Step 1: Convert the volumes of hydrogen and oxygen to moles.
To convert the volumes to moles, we will use the ideal gas law equation:
PV = nRT
Since the reaction occurs at standard temperature and pressure (STP), which is 0 degrees Celsius (273.15 K) and 1 atm pressure, we can use the following values:
Temperature (T) = 0 degrees Celsius + 273.15 K = 273.15 K
Pressure (P) = 1 atm
For hydrogen (H₂):
Volume (V) = 3 L
R is the ideal gas constant, which has a value of 0.0821 L·atm/(K·mol)
Plugging in these values into the ideal gas law equation, we can solve for moles (n):
n(H₂) = PV / RT
n(H₂) = (1 atm * 3 L) / (0.0821 L·atm/(K·mol) * 273.15 K)
n(H₂) ≈ 0.132 moles of hydrogen
For oxygen (O₂):
Volume (V) = 1.5 L
Using the same ideal gas law equation, we can solve for moles (n):
n(O₂) = PV / RT
n(O₂) = (1 atm * 1.5 L) / (0.0821 L·atm/(K·mol) * 273.15 K)
n(O₂) ≈ 0.0981 moles of oxygen
Step 2: Determine the moles of water formed.
From the balanced chemical equation, we can see that for every 2 moles of hydrogen, we produce 2 moles of water.
Since the mole ratio is 1:1 between hydrogen and water, the number of moles of water formed will be the same as the moles of hydrogen used. Therefore,
moles of water = moles of hydrogen = 0.132 moles
So, approximately 0.132 moles of water are formed.
Step 3: Find the volume of water at a temperature of 100 degrees Celsius and 1 atm pressure.
To find the gas volume of water when given the temperature and pressure, we'll use the ideal gas law equation again:
PV = nRT
Given:
Temperature (T) = 100 degrees Celsius + 273.15 K = 373.15 K
Pressure (P) = 1 atm
Moles of water (n) = 0.132 moles (from the previous step)
V = nRT / P
V = (0.132 mol * 0.0821 L·atm/(K·mol) * 373.15 K) / 1 atm
V ≈ 4.65184 L
Therefore, at a temperature of 100 degrees Celsius and 1 atm pressure, the gas volume of water is approximately 4.65184 L.