Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
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)+3H2(g)
In a particular reaction, 25.5 L of methane gas (measured at a
pressure of 736 torr and a temperature of 25 ?C) is mixed with 22.6
L of water vapor (measured at a pressure of 700 torrand a
temperature of 125 ?C). The reaction produces 27.0 L of hydrogen
gas measured at STP. What is the percent yield of the reaction?
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Hydrogen gas (a potential future fuel) can be formed by the
reaction of methane with water...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation CH (9) + H2O(g) → CO(g) + 3H2(g) In a particular reaction, 25.0 L of methane gas (measured at a pressure of 730 torr and a temperature of 25 °C) is mixed with 220 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 °C). The reaction produces 26.0 L of hydrogen gas...
An equilibrium mixture of water vapor, methane, carbon monoxide, and hydrogen at 1400 K has the...
An equilibrium mixture of water vapor, methane, carbon monoxide, and hydrogen at 1400 K has the composition: [H2O] = 9.0 M, [CH4] = 8.0 M, [CO] = 2.0 M, [H2] = 6.0 M, for the equilibrium, H2O(g) + CH4(g) ↔ CO(g) +3H2(g). If the initial reaction mixture was composed only of water vapor and methane gas, what was the initial concentration of the methane in molarity units?
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4...
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H2O(g) = 3H2(g) + CO (g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.13 M; H20,0.239 M; CO, 0.136 M; H2 1.21 M, at a temperature of 760 °C?
Question 8 10 pts Methane gas reacts with water vapor to produce a mixture of carbon...
Question 8 10 pts Methane gas reacts with water vapor to produce a mixture of carbon monoxide and hydrogen, according to the balanced equation below. CH4(8) + H2O(g) → CO(g) + 3H2(8) AH® for the reaction is +206.1 kJ/mol, while ASⓇ is +215 J/Komol. At what temperature (in °C) does this reaction become spontaneous?
1. Calculate the volume of hydrogen gas produced from the reaction of 0.832 g of aluminum...
1. Calculate the volume of hydrogen gas produced from the reaction of 0.832 g of aluminum when completely reacted with excess hydrochloric acid. The gas was collected over water at 25.0 C and a barometric pressure of 736 torr. 2Al (s) + 6HCl (aq) --> 2AlCl3 (aq) + 3H2 (g) 2. What mass of KClO3 decomposed to produce 325 mL of O2 gas at STP. 2KClO3 (s) --> 2KCl (s) + 3O2 (g)
Example At elevated temperatures, methane (CHA) reacts with water to produce hydrogen and carbon monoxide in...
Example At elevated temperatures, methane (CHA) reacts with water to produce hydrogen and carbon monoxide in what is known as a steam-reforming reaction: CH4(9)+H2O(g)= CO(g)+3H2(g) K= 2.4 x 10-4 at 900 K. Huge amounts of hydrogen are produced from natural gas in this way and are then used for the industrial synthesis of ammonia. If 1.2 x 10-2 mol of CH4, 8.0 x 10-3 mol of H20, 1.6 x 10-2 mol of CO, and 6.0 × 10-3 mol of H2...
Under certain circumstances, carbon dioxide, CO2(g), can be made to react with hydrogen gas, H2(g), to produce methane,...
Under certain circumstances, carbon dioxide, CO2(g), can be made to react with hydrogen gas, H2(g), to produce methane, CH4(g), and water vapor, H2O(g): CO2(g)+4H2(g)→CH4(g)+2H2O(g) How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 53.6 moles of water vapor? Express your answer with the appropriate units. For example, write the unit moles as mol.
9. Bond Energy. Hydrogen gas can hydrogen gas can be made by the reaction of methane...
9. Bond Energy. Hydrogen gas can hydrogen gas can be made by the reaction of methane gas and steam. CH4(8) + 2 H2O(g) → 4 H2(g) + CO2(g) Use the bond energies (Table 9.3 and Table 9.4) to gies (Table 9.3 and Table 9.4) to calculate AHan for the above reaction. (note: you need to write the Lewis structure to show how the atoms are bonded and is structure to show how the atoms are bonded and the types of...
a sample of hydrogen gas is mixed with water vapor. the mixture has a total pressure...
a sample of hydrogen gas is mixed with water vapor. the mixture has a total pressure of 755 torr and the water vapor has a partial pressure of 24 torr. what amount (in moles) of hydrogen gas is contained in 1.55 L of this mixture at 298 K?
Quizzes Question 3 How many liters of hydrogen gas are formed from the complete reaction of...
Quizzes Question 3 How many liters of hydrogen gas are formed from the complete reaction of 15.5g C? C(s) + H2O(g) --> CO(g)+ H2(g) Assume that the hydrogen gas is collected at a pressure of 1.00 atm and a temperature of 27.0 C. 2.86 L 31.8L 388L None of the above 38.0L Question 4 A gas is compressed from an initial volume of 3.33L to final volume of 0.22L by an external pressure of 0.50 atm. compression the gas releases...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation CH (9) + H2O(g) → CO(g) + 3H2(g) In a particular reaction, 25.0 L of methane gas (measured at a pressure of 730 torr and a temperature of 25 °C) is mixed with 220 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 °C). The reaction produces 26.0 L of hydrogen gas...
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H2O(g) = 3H2(g) + CO (g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.13 M; H20,0.239 M; CO, 0.136 M; H2 1.21 M, at a temperature of 760 °C?
Question 8 10 pts Methane gas reacts with water vapor to produce a mixture of carbon monoxide and hydrogen, according to the balanced equation below. CH4(8) + H2O(g) → CO(g) + 3H2(8) AH® for the reaction is +206.1 kJ/mol, while ASⓇ is +215 J/Komol. At what temperature (in °C) does this reaction become spontaneous?
Example At elevated temperatures, methane (CHA) reacts with water to produce hydrogen and carbon monoxide in what is known as a steam-reforming reaction: CH4(9)+H2O(g)= CO(g)+3H2(g) K= 2.4 x 10-4 at 900 K. Huge amounts of hydrogen are produced from natural gas in this way and are then used for the industrial synthesis of ammonia. If 1.2 x 10-2 mol of CH4, 8.0 x 10-3 mol of H20, 1.6 x 10-2 mol of CO, and 6.0 × 10-3 mol of H2...
9. Bond Energy. Hydrogen gas can hydrogen gas can be made by the reaction of methane gas and steam. CH4(8) + 2 H2O(g) → 4 H2(g) + CO2(g) Use the bond energies (Table 9.3 and Table 9.4) to gies (Table 9.3 and Table 9.4) to calculate AHan for the above reaction. (note: you need to write the Lewis structure to show how the atoms are bonded and is structure to show how the atoms are bonded and the types of...
Quizzes Question 3 How many liters of hydrogen gas are formed from the complete reaction of 15.5g C? C(s) + H2O(g) --> CO(g)+ H2(g) Assume that the hydrogen gas is collected at a pressure of 1.00 atm and a temperature of 27.0 C. 2.86 L 31.8L 388L None of the above 38.0L Question 4 A gas is compressed from an initial volume of 3.33L to final volume of 0.22L by an external pressure of 0.50 atm. compression the gas releases...
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