객관식
How many moles of carbon are needed to react with 525 g of hematite (Fe2O3) in the following reaction: Fe2O3 + 3C → 2Fe + 3CO?
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3. Chemical Reactions
Stoichiometry
객관식
Hydrogen gas can be formed by the reaction of methane with water according to the equation: CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g). In a particular reaction, 25.5 L of methane gas (measured at a pressure of 730 torr and a temperature of 298 K) is used. How many liters of hydrogen gas are produced at the same conditions?
A
25.5 L
B
51.0 L
C
76.5 L
D
102.0 L
검증된 단계별 안내1
Identify the balanced chemical equation for the reaction: CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g). This indicates that 1 mole of CH4 produces 3 moles of H2.
Use the ideal gas law, PV = nRT, to calculate the number of moles of CH4. Convert the pressure from torr to atm by dividing by 760 (since 1 atm = 760 torr).
Calculate the number of moles of CH4 using the formula: n = PV / RT, where P is the pressure in atm, V is the volume in liters, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
Determine the moles of H2 produced using the stoichiometry of the reaction. Since 1 mole of CH4 produces 3 moles of H2, multiply the moles of CH4 by 3 to find the moles of H2.
Convert the moles of H2 back to volume using the ideal gas law, assuming the same conditions of temperature and pressure. Use the formula V = nRT / P to find the volume of H2 produced.
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