Hydrogen cyanide is produced industrially from ammonia and methane at 1000ºC utilizing a platinum-rhodium catalyst by...
Hydrogen cyanide is produced industrially from ammonia and methane at 1000ºC utilizing a platinum-rhodium catalyst by the following reaction: 2 NH3(g) + 3 O2(g) + 2 CH4(g) → 2 HCN(g) + 6 H2O(g)
a) Calculate ΔGº, ΔHº, and ΔSº for this reaction at 25.00ºC. ΔGº ΔHº ΔSº
b) Why is this reaction performed at such a high temperature (1000ºC)? _____________________________________________________________________________ _____________________________________________________________________________
c) Calculate the value of the equilibrium constant for this reaction at 25.00ºC. ___________________________________
d) What is the value of ΔG at 25.00ºC if each of the gases is at a partial pressure of 0.25 atm.? ___________________________________
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Hydrogen cyanide is produced industrially from ammonia and
methane at 1000ºC utilizing a platinum-rhodium catalyst by...
Identify limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen. 2CH4...
Identify limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen. 2CH4 (g) + 2NH3(g) + 302 (g) —2HCN (g) + 6H20 (1) Determine the limiting reactant in a mixture containing 175 g of CH4, 160 g of NH3, and 607 g of O2. Calculate the maximum mass (in grams) of hydrogen cyanide, HCN, that can be produced in the reaction. The limiting reactant is: CH4 O2 NH3 Amount of HCN formed = g
Hydrogen cyanide is used in the manufacture of clear plastics such as Plexiglas. It is prepared from ammonia (NH3) and methane (CH4) according to the following reaction. a. Calculate the value of q i...
Hydrogen cyanide is used in the manufacture of clear plastics such as Plexiglas. It is prepared from ammonia (NH3) and methane (CH4) according to the following reaction. a. Calculate the value of q if 3.855 grams of ammonia react with excess oxygen and 5. methane b. Calculate the value of q if 4.394 grams of oxygen react with excess ammonia and methane. Calculate the value of q if 2.475 grams of methane reacts with excess oxygen and ammonia Calculate the...
Calculate the value of the free energy change, ΔG, for the reaction below at 227.0ºC when...
Calculate the value of the free energy change, ΔG, for the reaction below at 227.0ºC when the pressures of NO (g) = 2.00 atm, O₂ (g) = 10.00 atm, and NO₂ (g) = 0.0250 atm. 2 NO (g) + O₂ (g) → 2 NO₂ (g) ΔGº = -70.54 kJ ΔHº = -114.14 kJ ΔSº = -146.43 J/K ΔG = ? kJ
Calculate the value of the free energy change, ΔG, for the reaction below at 175.0ºC when...
Calculate the value of the free energy change, ΔG, for the reaction below at 175.0ºC when the pressures of H2S (g) = 0.0100 atm, SO2(g) = 0.0250 atm, and H2O (g) = 2.50 atm. 2 H2S (g) + SO2 (g) → 3 S (s) + 2 H2O (g) ΔGº = –90.88 kJ ΔHº = –146.47 kJ ΔSº = –186.45 J/K
Identity limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen 2CH,...
Identity limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen 2CH, (g) + 2NH3 (9) +302 (9) —2HCN) + 6H20 (1) Determine the limiting reactant in a mixture containing 129 g of CH, 152 g of NH3, and 348 g of Oz Calculate the maximum mass (in grams) of hydrogen cyanide, HCN, that can be produced in the reaction The limiting reactant is. OCH4 O NH3 Amount of HCN formed
Hydrogen cyanide gas can be produced by the following reaction: 2 CH4(g) + 2 NH3(g) +...
Hydrogen cyanide gas can be produced by the following
reaction:
2 CH4(g) + 2 NH3(g) + 3 O2(g)
2 HCN(g) + 6 H2O(g)
A) what volume of oxygen gas (in L) is required to react
completely to produce 550 L of hydrogen cyanide? Assume reactant
and product volumes are measured at 300 kPa and 1200 degree
Celcius.
B) what volume of water vapour (in L) will be produced during
the production 255 L of hydrogen cyanide? Assume all reactant and...
Please help with these questions 1. Methane (CH4) burns in air to form carbon dioxide and...
Please help with these questions
1. Methane (CH4) burns in air to form carbon dioxide
and water as shown below.
CH4(g) + 2 O2(g) → CO2(g) + 2
H2O(l)
If a sample of methane occupies 802. mL at 3.23 atm, what
pressure (in atm) of oxygen gas with the same temperature and
volume is required to complete the reaction?
2. Consider the reaction between hydrogen gas and nitrogen gas
to form ammonia:
3 H2(g) + N2(g) → 2 NH3(g).
What...
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction 2NH3(g)+CO2(g)→NH2CONH2(aq)+H2O(l) Given that ΔG∘...
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction 2NH3(g)+CO2(g)→NH2CONH2(aq)+H2O(l) Given that ΔG∘ = -13.6 kJ, calculate ΔG at 25 ∘C for the following sets of conditions. (Figure 1) 1) 20 atm NH3, 20 atm CO2, 4.0 M NH2CONH2 2) 9.0×10−2 atm NH3, 9.0×10−2 atm CO2, 1.0 M NH2CONH2 Is the reaction spontaneous for the conditions in part (a) and/or part (b)? spontaneous for the conditions in part (b), nonspontaneous for the conditions in part (a) nonspontaneous...
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the following reaction: 2NH3(g)+CO2(g)→...
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the following reaction: 2NH3(g)+CO2(g)→NH2CONH2(aq)+H2O(l) Given that ΔG∘ = −13.6 kJ/mol, calculate ΔG at 25∘C for the following sets of conditions Part A 50 atm NH3, 50 atm CO2, 4.0 M NH2CONH2 Express the free energy in kilojoules per mole to two significant figures. Part B 8.0×10−2 atm NH3, 8.0×10−2 atm CO2, 1.0 M NH2CONH2 Express the free energy in kilojoules per mole to two significant figures. Part C Is the reaction spontaneous for the conditions in...
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for thi...
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is ________. -3.86 × 103 -1.8 -7.25 × 103 -104.5 -40.5
Identify limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen. 2CH4 (g) + 2NH3(g) + 302 (g) —2HCN (g) + 6H20 (1) Determine the limiting reactant in a mixture containing 175 g of CH4, 160 g of NH3, and 607 g of O2. Calculate the maximum mass (in grams) of hydrogen cyanide, HCN, that can be produced in the reaction. The limiting reactant is: CH4 O2 NH3 Amount of HCN formed = g
Hydrogen cyanide is used in the manufacture of clear plastics such as Plexiglas. It is prepared from ammonia (NH3) and methane (CH4) according to the following reaction. a. Calculate the value of q if 3.855 grams of ammonia react with excess oxygen and 5. methane b. Calculate the value of q if 4.394 grams of oxygen react with excess ammonia and methane. Calculate the value of q if 2.475 grams of methane reacts with excess oxygen and ammonia Calculate the...
Identity limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen 2CH, (g) + 2NH3 (9) +302 (9) —2HCN) + 6H20 (1) Determine the limiting reactant in a mixture containing 129 g of CH, 152 g of NH3, and 348 g of Oz Calculate the maximum mass (in grams) of hydrogen cyanide, HCN, that can be produced in the reaction The limiting reactant is. OCH4 O NH3 Amount of HCN formed
Hydrogen cyanide gas can be produced by the following
reaction:
2 CH4(g) + 2 NH3(g) + 3 O2(g)
2 HCN(g) + 6 H2O(g)
A) what volume of oxygen gas (in L) is required to react
completely to produce 550 L of hydrogen cyanide? Assume reactant
and product volumes are measured at 300 kPa and 1200 degree
Celcius.
B) what volume of water vapour (in L) will be produced during
the production 255 L of hydrogen cyanide? Assume all reactant and...
Please help with these questions
1. Methane (CH4) burns in air to form carbon dioxide
and water as shown below.
CH4(g) + 2 O2(g) → CO2(g) + 2
H2O(l)
If a sample of methane occupies 802. mL at 3.23 atm, what
pressure (in atm) of oxygen gas with the same temperature and
volume is required to complete the reaction?
2. Consider the reaction between hydrogen gas and nitrogen gas
to form ammonia:
3 H2(g) + N2(g) → 2 NH3(g).
What...
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