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?

Solutions

Expert Solution

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?

First calculate the moles of HCN:

1.5*10^5 kg *1000g / 1.0 kg / molar mass HCN, 27.0253 g / mole

= 5550354.668 moles HCN

Now, calculate the moles of NH3 as follows:

5550354.668 moles HCN * 2 mole NH3/ 2 mole HCN

= 5550354.668 moles NH3

Amount of NH3 = Number of moles * molar mass

= 5550354.668 moles NH3 * 17.031 g / mole

= 9.45*10^7 g

= 9.45*10^4 kg NH3

Here the reaction the reaction has a 97.5%

So, 9.45*10^4 kg NH3 / 0.975= 9.695*10^4 kg NH3

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

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?

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?

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

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...

For the reaction below (an undesired side reaction in the industrial production of nitric acid), if...

For the reaction below (an undesired side reaction in the industrial production of nitric acid), if you begin by adding 0.0150 moles of both NH3 and O2 to a 1.00 L reaction vessel, and once equilibrium is established you have a nitrogen concentration of 0.00196 M, what is the value for Kc? 4 NH3 (g) + 3 O2 (g) <--> 2 N2 (g) + 6 H2O (g)

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...

What is the balanced equation for the reaction of, Hydrogen cyanide from ammonia and methane gas...

What is the balanced equation for the reaction of, Hydrogen cyanide from ammonia and methane gas (Degussa process) CH4(g) + NH3(g) -> HCN (g) + 3 H2(g)? Determine the ΔH, ΔS, and ΔG at 298 K.

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...

1. Calculate the enthalpy change for the reaction based ion the given information: 2CH4(g) + 2O2(g) -->...

1. Calculate the enthalpy change for the reaction based ion the given information: 2CH4(g) + 2O2(g) --> CH2CO(g) + 3H2O(g) CH2CO(g) + 2O2(g) --> 2CO2(g) + H2O(g) Delta H = -941.1 kJ CH4(g) + 2O2(g) --> CO2(g) + 2H2O(g) Delta H = -882.3 kJ 2. Suppose a large size chocolate fudge ice cream gives 162 Calories. If an ice cream contains 6.00 g of carbohydrate and 12.0 g of protein then find out grams of fat? [1g Fat = 9kcal, 1g...

1. Calculate the enthalpy change for the reaction based ion the given information: 2CH4(g) + 2O2(g) -->...

Subjects