If 25grams of methane, CH4, and 30g of ammonia, NH3, are combined with excess oxygen, how much...
2CH4 + 2NH3 + 3O2 -> 2HCN + 6H2O
Homework Answers
The first thing you need to determine is which of either methane or ammonia is the limiting reagent. To do so, the following calculations need to beperformed:
There are less moles of methane, therefore it is the limiting reagent. This means that there will be no methane left, but some ammonia left. Now youneed to calculate the quantity of ammonia that will be left over.
Since methane and ammonia react in a 2 to 2 molar ratio (which reduces to 1 to 1), there will be about 0.2 moles of ammonia left.
Now calculate the mass of ammonia contained in 0.20 moles.
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If 25grams of methane, CH4, and 30g of ammonia, NH3, are combined with excess oxygen, how much...
Use standard enthalpies of formation to determine ?Horxnfor: 2NH3(g) + 3O2(g) + 2CH4(g) ?...
Use standard enthalpies of formation to determine ΔHorxnfor:2NH3(g) + 3O2(g) + 2CH4(g) → 2HCN(g) + 6H2O(g)Enter in kJ.
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...
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
HCN is a highly toxic gas and can be formed at high temperatures in the following...
HCN is a highly toxic gas and can be formed at high temperatures in the following reaction: 2CH4 (g) + 3O2 (g) + 2NH3 (g) → 2HCN(g) + 6H2O (g) a) How many litres of CH4 (g), O2 (g) and NH3 (g) are needed to produce 15 litres of HCN (g)? b) How many litres of water will be produced in this reaction? Please explain where you get all your values from and your working out.
Want 2CH4 + 2NH3 ----> 2HCN + 6H2 From: N2+3H2 --->2NH3 DeltaH: -91.8KJ 2H2+C--->CH4 DeltaH:...
Want 2CH4 + 2NH3 ----> 2HCN + 6H2 From: N2+3H2 --->2NH3 DeltaH: -91.8KJ 2H2+C--->CH4 DeltaH: -74.9 KJ 2C+H2+N2----> 2HCN DeltaH: 270.3 KJ
Use standard enthalpies of formation to determine ΔHorxn for: 1. 3NO2(g) + H2O(l) → 2HNO3(aq) +...
Use standard enthalpies of formation to determine ΔHorxn for: 1. 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) (Enter in kJ.) 2. Find the change in internal energy for this reaction. Enter in kJ. Use standard enthalpies of formation to determine ΔHorxnfor: 3. 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) (Enter in kJ.) 4. Find the change in internal energy for this reaction. Enter in kJ. Use standard enthalpies of formation to determine ΔHorxn for: 5. 2NH3(g) + 3O2(g) + 2CH4(g)...
2NH3(g) + 3O2(g) +2CH4(g) 2HCN(g) +6H2O(g)?H°f (kJ mol-1)S° (J K-1 mol-1)NH3(g)...
2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(g)?H°f (kJ mol-1)S° (J K-1 mol-1)NH3(g)-46193O2(g)0205CH4(g)-75186HCN(g)135.1202H2O(g)-242189The above reaction is used in the industrial production of hydrogen cyanide. (The tabulated values ?H°fand S° are for 25°C. For the purposes of this question assume that ?H° and ?S° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.)?H° is -939.8?S° is 165Calculate ?G° at 1005°C, for this equation.Are the following statements about this process True...
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
You are investigating how methane (CH4) and ammonia (NH3) combine to generate cyanamide (H2NCN) and hydrogen...
You are investigating how methane (CH4) and ammonia (NH3) combine to generate cyanamide (H2NCN) and hydrogen gas H2) according to the following reaction: CH4(g) + 2NH3(g) → H2NCN(g) + 4H2(g) The lab's temperature on the day of the experiment is 24 ºC and the barometer is reading 753 mmHg. If you need to produce 0.455 grams of H2, what is the minimum volume of methane that is required? The minimum volume of methane needed is [V]
Acrylonitrile, C3H3N, is an important industrial chemical. Propene, C3H6, reacts with ammonia & oxygen in the...
Acrylonitrile, C3H3N, is an important industrial chemical. Propene, C3H6, reacts with ammonia & oxygen in the gas phase to produce acrylonitrile and water vapor according to the following balanced chemical equation. 150 g of propene was reacted with 270.0 L ammonia & excess oxygen (both STP). 175g of C3H3N was isolated after the reaction. C3H6(g) + 2NH3(g) + 3O2(g) -> 2 C3H3N(l) + 6H2O(g) MM: 42.080 17.0304 31.9988 53.0634 1 8.0153 (a) Calculate the theoretical yield of acrylonitrile based...
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...
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
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
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