CH4(g) + H2O(g) → CO(g) + 3 H2 (g)
Calculate how much H2(g) is produced from each reactant:
H2(g) from CH4(g):
P = 0.9658 atm
V = 26.0 L
T = 25°C + 273.15 = 298.15 K
nCH4 = 1.0263 mol
moles H2 = 3.079 mol
H2(g) from H2O(g):
22.6 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 oC
P = 0.9263 atm
V = 22.6 L
T = 125°C + 273.15 = 398.15 K
nH2O = 0.6407 mol
moles H2 = 1.922 mol
H2O(g): produces a smaller amount of H2(g) → H2O(g) is the limiting reactant
theoretical yield = 1.922 mol H2
Calculate the theoretical yield of H2(g) (volume):
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation:
CH4(g) + H2O(g) → CO(g) + 3 H2 (g)
In a particular reaction, 26.0 L of methane gas (measured at a pressure of 734 torr and a temperature of 25 oC) is mixed with 22.6 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 oC). The reaction produces 26.6 L of hydrogen gas measured at STP.
What is the percent yield of the reaction?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Standard Temperature and Pressure concept. You can view video lessons to learn Standard Temperature and Pressure. Or if you need more Standard Temperature and Pressure practice, you can also practice Standard Temperature and Pressure practice problems.