Ammonia reacts with oxygen to form nitric oxide and water
vapor:
4NH3 + 5O2 ---> 4NO +
6H2O
When 20.0 g NH3 and 50.0 g O2 are allowed to react,
which is the limiting reagent?
A) NO
B) O2
C) H2O
D) no reagent is limiting
E) NH3
What is the coefficient for O2 when the following
combustion reaction of a hydrocarbon is balanced?
___C7H14 + ___ O2 ---> ___
CO2 + __ H2O
A) none of these
B) 10
C) 11
D) 21
E) 42
4 NH3 + 5 O2 → 4 NO + 6 H2O
Let's assume for the moment that ammonia is the limiting reactant.
Let's calculate the mass of oxygen that would be required to react
completely with 20.0 g of ammonia. We can use dimensional analysis
and equation coefficients to convert 20.0 g of NH3 to moles of NH3,
to moles of O2, to grams of O2. We shall need the following
equalities to set up conversion factors:
1 mol NH3 = 17.03052 g NH3
4 mol NH3 = 5 mol O2
1 mol O2 = 31.9988 g O2
[(20.0 g NH3)/1][(1 mol NH3)/(17.03052 g NH3)][(5 mol O2)/(4 mol
NH3)][(31.9988 g O2)/(1 mol O2)] = 46.972724 g O2
Answer: Since only 46.972724 grams of oxygen is required, and as
much as 50.0 grams of oxygen is available, oxygen is in excess, and
ammonia is the limiting reactant indeed
E)Ammonia
2C7H14 + 21O2 -> 14CO2 + 14H2O
D)21
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 ---> 4NO...
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 +5O2 → 4NO + 6H2O What is the theoretical yield of water, in moles, when 40.0g NH3 and 50.0g O2 are mixed and allowed to react: 1.87 mol 3.53 mol 1.57 mol 1.30 mol None of these
Always show your work. No credit will be given for any answers (even if they are correct) for which work is not shown. Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor: 4NH3 + 502 ---> 4NO + 6H2O What is the theoretical yield of water, in moles, when 40.0 g NH3 and 50.0g, O2 are mixed and allowed to react?
1) Ammonia, NH3, reacts with molecular oxygen, O2, to form nitric oxide, NO, and water:4NH3(g) + 5O2(g) = 4NO (g) +6H2O(l)A. What is the limiting reactant and what is the theoretical yield of NO?B. What is the theoretical yield of H2O?C. How many grams of excess reagent will be left over?D. If the actual yield of NO had been 91 g, what would be the percent yield of the reaction
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) In a certain experiment, 1.85 g of NH3 reacts with 3.39 g of O2. 1) How many grams of NO and of H2O form? 2) How many grams of the excess reactant remain after the limiting reactant is completely consumed?
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) In a certain experiment, 2.05 g of NH3 reacts with 3.76 g of O2. How many grams of NO and of H2O form? Enter your answers numerically separated by a comma.
1. Ammonia reacts with oxygen according to the equation 4NH3(g)+5O2(g)→4NO(g)+6H2O(g),ΔHrxn=−906 kJ Calculate the heat (in kJ) associated with the complete reaction of 155 g of NH3. 2. What mass of butane in grams is necessary to produce 1.5×103 kJ of heat? What mass of CO2 is produced? Assume the reaction to be as follows: C4H10(g)+132O2(g)→4CO2(g)+5H2O(g),ΔHrxn=−2658 kJ
Part A Ammonia reacts with oxygen according to the equation 4NH3(g)+5O2(g)→4NO(g)+6H2O(g),ΔHrxn=−906 kJ Calculate the heat (in kJ) associated with the complete reaction of 155 g of NH3. Part B What mass of butane in grams is necessary to produce 1.5×103 kJ of heat? What mass of CO2 is produced? Assume the reaction to be as follows: C4H10(g)+132O2(g)→4CO2(g)+5H2O(g),ΔHrxn=−2658 kJ
The first step in the Oswald process for producing nitric acid is 4NH+5o2- 4NO + 6H2O if 132g of ammonia reacts with 132g of oxygen A) how many grams of nk itric oxide(No) will be produced B) which compound is limiting reagent C) what is the % yield of this reaction if actual yield of NO is 67.Og?
An Important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide according to the following balanced chemical equation. What is AHpxn for this reaction? 4NH3(g) + 5O2(g) -4NO(g) + 6H2O(9) Substance AH?f(kJ/mol) NH3(g) -46.3 NO(9) 90.3 H2O(9) -241.8 0 -1274.8 kJ/mol -904.4 kJ/mol 0 -240.2 kJ/mol 0 -197.8kJ 197.8 kJ/mol
How many grams of NO and of H2O form? Enter your answers numerically separated by a comma. How many grams of the excess reactant remain after the limiting reactant is completely consumed? One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) In a certain experiment, 1.50 g of NH3 reacts with 2.75 g of O2.