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8. One reaction that can be used to remove NO gas from power plant emission is...
When an exothermic reaction produces a gas, what can be done to allow the reaction to...
When an exothermic reaction produces a gas, what can be done to allow the reaction to continue to product once an equilibrium has been reached? Example: CH4 (g) + O2 (g) -> CO2 (g) + H20 (1) + Heat O Add more product O Apply more heat Reduce the amounts of reactants Remove gas to lower the pressure decrease the pressure
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...
Consider the following reaction. CH4(g) + 2 O2(g) - CO2(g) + 2 H20(1) AH = -891...
Consider the following reaction. CH4(g) + 2 O2(g) - CO2(g) + 2 H20(1) AH = -891 kJ Calculate the enthalpy change for each of the following cases. (a) 2.00 g methane is burned in excess oxygen. Гk (b) 2.00 x 103 L methane gas at 743 torr and 25°C is burned in excess oxygen.
Ynthesis gas, a mixture that includes the fuels carbon monoxide and molecular hydrogen, is used p...
ynthesis gas, a mixture that includes the fuels carbon monoxide and molecular hydrogen, is used produce liquid hydrocarbons and methanol. It is made at pressures up to 100 atm by oxidation of methane followed by the steam re-forming and water-gas shift reactions. Because the is exothermic, temperatures reach 950 1100°C, and the conditions are such that the amounts of hydrogen, carbon monoxide, carbon dioxide, methane and water leaving the reactor are close to the equilibrium amounts for the steam re-forming...
84. Hydrogen can be extracted from natural gas according to the reaction: CH4(8) + CO2(g) = 2 CO(g) + 2 H2(g) Ky =...
84. Hydrogen can be extracted from natural gas according to the reaction: CH4(8) + CO2(g) = 2 CO(g) + 2 H2(g) Ky = 4.5 x 102 at 825 K An 85.0-L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. Assuming ideal gas behavior, calcu- late the mass of H, (in g) present in the reaction mixture at equi- librium. What is the percent yield of the reaction under these conditions? CaO(s) :...
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...
8. i) How many moles of Neon gas will occupy a container with a volume of...
8. i) How many moles of Neon gas will occupy a container with a volume of 2.5 L at a temperature of 31.5°C and a pressure of 912 torr? ii) What is the density of the gas? 9. A tank of compressed mixed gases contains 0.40 moles of Hz (hydrogen), 1.3 moles of NO2 (nitrogen dioxide), and 0.80 moles of Ar (argon). The total pressure in the tank is 2.8 atm. What is the partial pressure of the Hz gas?...
The following data were obtained for the reaction of methane with oxygen: CH4(g) + 202(g) CO2(g)...
The following data were obtained for the reaction of methane with oxygen: CH4(g) + 202(g) CO2(g) + 2H20(1) → time(min)[CH4l (mol/L) 0 10 20 30 0.050 0.030 0.020 0.015 0.020 a) How many moles of CO2 are produced for each mole of CH4 that is used up? b) What concentration of CH4 is used up after 10 minutes? c) What is the concentration of carbon dioxide produced after 20 minutes? d) Write an equation for reaction rate in terms of...
Flue gas from a furnace is 30 mol% SO2, 25 mol% O2, and remainder CO2. To...
Flue gas from a furnace is 30 mol% SO2, 25 mol% O2, and remainder CO2. To clean 1155 mol/hr of flue gas and remove SO2, it is to be reacted with pure methane (natural gas) such that for every 65 moles of SO2 in the flue gas, 67 moles of methane is used (supplied). The primary reaction between methane and SO2 is as follows CH4 + SO2 → H2S + CO2 + H2O A side reaction also occurs as...
Methane (CH4) and oxygen (O2) react to form formaldehyde (CH2O) (reaction #1), with a competing side...
Methane (CH4) and oxygen (O2) react to form formaldehyde (CH2O) (reaction #1), with a competing side reaction (#2) in which methane and oxygen form carbon dioxide (CO2): CH4(v) + O2(g) -> CH2O(v) + H2O(l) (reaction #1) CH4(v) + 2O2(g) -> CO2(g) + 2H2O(l) (reaction #2) A fresh feed of an equimolar gas mixture of CH4 and O2 is combined with a recycle stream and fed to a reactor. The single-pass conversion of CH4 is 30% and the selectivity of CH2O...
When an exothermic reaction produces a gas, what can be done to allow the reaction to continue to product once an equilibrium has been reached? Example: CH4 (g) + O2 (g) -> CO2 (g) + H20 (1) + Heat O Add more product O Apply more heat Reduce the amounts of reactants Remove gas to lower the pressure decrease the pressure
Consider the following reaction. CH4(g) + 2 O2(g) - CO2(g) + 2 H20(1) AH = -891 kJ Calculate the enthalpy change for each of the following cases. (a) 2.00 g methane is burned in excess oxygen. Гk (b) 2.00 x 103 L methane gas at 743 torr and 25°C is burned in excess oxygen.
ynthesis gas, a mixture that includes the fuels carbon monoxide and molecular hydrogen, is used produce liquid hydrocarbons and methanol. It is made at pressures up to 100 atm by oxidation of methane followed by the steam re-forming and water-gas shift reactions. Because the is exothermic, temperatures reach 950 1100°C, and the conditions are such that the amounts of hydrogen, carbon monoxide, carbon dioxide, methane and water leaving the reactor are close to the equilibrium amounts for the steam re-forming...
84. Hydrogen can be extracted from natural gas according to the reaction: CH4(8) + CO2(g) = 2 CO(g) + 2 H2(g) Ky = 4.5 x 102 at 825 K An 85.0-L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. Assuming ideal gas behavior, calcu- late the mass of H, (in g) present in the reaction mixture at equi- librium. What is the percent yield of the reaction under these conditions? CaO(s) :...
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...
8. i) How many moles of Neon gas will occupy a container with a volume of 2.5 L at a temperature of 31.5°C and a pressure of 912 torr? ii) What is the density of the gas? 9. A tank of compressed mixed gases contains 0.40 moles of Hz (hydrogen), 1.3 moles of NO2 (nitrogen dioxide), and 0.80 moles of Ar (argon). The total pressure in the tank is 2.8 atm. What is the partial pressure of the Hz gas?...
The following data were obtained for the reaction of methane with oxygen: CH4(g) + 202(g) CO2(g) + 2H20(1) → time(min)[CH4l (mol/L) 0 10 20 30 0.050 0.030 0.020 0.015 0.020 a) How many moles of CO2 are produced for each mole of CH4 that is used up? b) What concentration of CH4 is used up after 10 minutes? c) What is the concentration of carbon dioxide produced after 20 minutes? d) Write an equation for reaction rate in terms of...
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