Question
In: Chemistry
Hydrogen cyanide, a highly toxic compound, is made by the following reaction: 2CH4(g) + 2 NH3(g)...
Hydrogen cyanide, a highly toxic compound, is made by the
following reaction:
2CH4(g) + 2 NH3(g) + 3
O2(g) → 2 HCN(g) + 6
H2O(g) What is the limiting reagent if 639.7g
of O2 are added to 429.3g of NH3(with excess
CH4)?
[O2]
A. What is the mass of HCN that can be produced from these reactants? ___ g
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Hydrogen cyanide, a highly toxic compound, is made by the following reaction: 2CH4(g) + 2NH3(g) +...
Hydrogen cyanide, a highly toxic compound, is made by the
following reaction:
2CH4(g) + 2NH3(g) +
3O2(g) → 2HCN(g) +
6H2O(g)
Given that there is 25.9 g of O2 are added to 44.8 g
of NH3(with excess CH4), What is the mass of
HCN that can be produced from these reactants?
The reaction for the industrial production of hydrogen cyanide is given below. 2CH4 + 2NH3 +...
The reaction for the industrial production of hydrogen cyanide
is given below.
2CH4 + 2NH3 + 3O2 --> 2HCN + 6H2O
What mass of NH3 is required for the synthesis of 1.5 × 10^5 kg
of HCN if the reaction has a 97.5% yield?
The reaction for the industrial production of hydrogen cyanide is given below. 2CH4 + 2NH3 +...
The reaction for the industrial production of hydrogen cyanide
is given below.
2CH4 + 2NH3 + 3O2 --> 2HCN + 6H2O
What mass of NH3 is required for the synthesis of 1.5 × 105 kg
of HCN if the reaction has a 97.5% yield?
Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane. 2 NH3(g)...
Hydrogen cyanide is produced industrially from the reaction of
gaseous ammonia, oxygen, and methane.
2 NH3(g) + 3 O2(g) + 2
CH4(g) → 2 HCN(g) + 6
H2O(g)
If 5.29 ✕ 103 kg each of NH3,
O2, and CH4 are reacted, what mass of HCN and
of H2O will be produced, assuming 100% yield?
HCN
g
H2O
g
A solution is prepared by dissolving 14.4 g ammonium sulfate in
enough water to make 113.0 mL of stock solution. A 13.20-mL...
Hydrogen cyanide gas (HCN), a powerful respiratory inhibitor, is highly toxic. It is a very weak...
Hydrogen cyanide gas (HCN), a powerful respiratory inhibitor, is
highly toxic. It is a very weak acid (Ka = 6.2 x 10-10) when
dissolved in water. If a 50.0 ml sample of 0.100 M HCN is titrated
with 0.100 M NaOH, calculate the pH of the solution After 8.00 mL
of 0.100 M NaOH has been added At the halfway point of the
titration At the equivalence point of the titration
Hydrogen cyanide is a highly poisonous substance that can be prepared by the reaction of methane...
Hydrogen cyanide is a highly poisonous substance that can be
prepared by the reaction of methane and ammonia:
CH4 (g) + NH3 (g) → HCN(g) + 3 H2 (g)
What is the heat of reaction at constant pressure? Provide an
answer correct to 3 significant figures. Do not use scientific
notation or include units to report your answer. You do need to
include the sign as a part of your answer.
N2 (g) + 3 H2 (g) → 2 NH3...
Hydrogen cyanide can be produced by the Andrussov process 2 CH4 + 2 NH3 + 3...
Hydrogen cyanide can be produced
by the Andrussov process
2 CH4 + 2 NH3 + 3 O2 + --> 2 HCN + 6
H2O
What mass of water, H2O, can be produced from the
reaction of 175 kg methane, CH4?
What percentage of resulted Hydrogen in the reaction: CH4 (g) + NH3 (g) --> HCN (g)...
What percentage of resulted Hydrogen in the reaction:
CH4 (g) + NH3 (g) --> HCN (g) + 3H2 (g) must be burnt, with
formation if H2O (g), to ensure the quantity of heat absorbed in
the reaction?
(the answer is: approximately 35%)
Heat of formation : Hf (kJ/mol)
CH4 (g) = -74,7
NH3 (g) = -46,2
HCN (g) = 130,5
H2O (g) = -241,6
The compound acrylonitrile can be made in the following reaction: 2C3H6(g) + 2NH3(g) + 3O2(g) →...
The compound acrylonitrile can be made in the following
reaction: 2C3H6(g) + 2NH3(g) + 3O2(g) → 2C3H3N(g) + 6H2O(g) A 250.0
L reaction vessel is charged to the following partial pressures at
500°C: PC3H6 = 10.0 atm PNH3 = 12.0 atm PO2 = 9.0 atm
A) What is the total pressure in the vessel just after the
reagent gases are added (assume ideal behavior)?
B) What are the mole ratios of the reagent gases in the vessel
before the reaction...
5a. Hydrogen cyanide is produced in the following balancedequation: 2NH3 (g) + 3O2 (g) +...
5a. Hydrogen cyanide is produced in the following balanced
equation: 2NH3 (g) + 3O2 (g) + 2 CH4 (g) → 2HCN (g) + 6 H2O (g).
Given the standard heats of formation: ∆H o f (kJ/mol) NH3
(g) - 46, CH4 (g) -75, HCN (g) 135, H2O (g) -242 Calculate
the approximate H of this reaction.5b. Given: Cu2O (s) + ½ O2 (g) → 2 CuO (s) H = -144 kJ2Cu2O (s) → 2Cu(s) + 2CuO (s) H = 22...
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