When 10.0 mol of ammonia and 10.0 mol of oxygen gas are transferred into a 10.0-

Question

When 10.0 mol of ammonia and 10.0 mol of oxygen gas are transferred into a 10.0-L container at 0.00 C and burn, nitrogen monoxide and water are produced. Then, the products return to 0.00 C slowly so volume and vapor pressure of ice (solid water) are ignored.NH3(g) + O2(g) = NO(g) + H2O(s) [unbalanced, at 0.00 C]

a. what is the total pressure of the vessel before the reaction?

b. balance the equation above

c. the limiting reactant is___, and the excess reactant is___

d. how many moles of nitrogen monoxide are present

e. what is the amount in moles of the excess reactant left over remaning in the contianer

f. what is the pressure reamining in the vessel

g. what is the pressure difference

Explanation / Answer

a) what is the total pressure of the vessel before the reaction?

Partial molar Pressure of Ammonia = PV = nRT

R = Gas constant = 0.082057 L atm mol-1K-1

P =?, V= 10 L, n = 10 mol, T =0 C = 273 K

Hence P = nRT/V = 10mole x 0.082057 L atm mol-1K-1 x 273 K / 10 L = 22.4 atm

Similarly calculated for Oxygen = 22.4 atm

Toatl Pressure = 44.8 atm

b) balance the equation above

     8 NH3 + 10 O2 --> 8 NO + 12 H2O

c) The limiting reactant is Oxygen, and the excess reactant is Ammonia.

d) how many moles of nitrogen monoxide are present

   Ans: 8 moles

e) what is the amount in moles of the excess reactant left over remaning in the contianer

    Ans: 2 moles of Ammonia

f) what is the pressure reamining in the vessel

Ans: P = nRT/V = 10 mole x 0.082057 L atm mol-1K-1 x 273 K / 10 L = 22.4 atm

g) Pressure difference = 22.4 atm

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