1. How many moles of CO2 are produced when 2.5 moles of O2 react according to th
ID: 304049 • Letter: 1
Question
1. How many moles of CO2 are produced when 2.5 moles of O2 react according to the following equation?
C3H8 + 5O2 ? 2FeO + 3SO2
2. How many grams of fluorine are required to produce 40.0 g of FeF3 from the reaction shown below?
2Fe + 3F2 ? 2FeF3
3. Consider the reaction N2+O2 ? 2NO if we react 25.00 grams of nitrogen with 35.00 grams of oxygen, how many grams of NO will be produced and what is the limiting reagent in this reaction?
4. The reaction N2+3H2 ? 2NH3 is used to produce ammonia. When 650.0 grams of hydrogen was reacted with nitrogen, 1575 grams of ammonia were produced. What is the percent tield of this reaction?
5. What is the mole ratio of Fe2S3 to O2 in the equation below?
Fe2S3 + 4O2 2FeO + 3SO2
Explanation / Answer
In Question 1 the given equation is wrong and it is modified here.
Balanced equation:
C3H8 + 5 O2 ====> 3 CO2 + 4 H2O
Reaction type: combustion
moles of O2 reacted = 2.5 Moles
Moles of CO2 produced = 1.5
Hence 1.5 Moles of CO2 will be produced
Question 2
Balanced equation
2 Fe + 3 F2 ===> 2 FeF3
Reaction type: synthesis
40.0 g of FeF3 = 40 / 112.84 = 0.3544 Moles
Moles of fluorine are required = 0.53172 Moles
grams of fluorine are required = 0.53172 x 37.99 = 20.203 gm
Qusetion 3
Balanced equation:
N2 + O2 ====> 2 NO
Reaction type: synthesis
25.00 grams of nitrogen = 25 / 28 = 0.8924 Moles
35.00 grams of oxygen = 35 / 32 = 1.093 Moles
Limiting reagent is Nitrogen
grams of NO will be produced = 1.784 x 30.00 = 53.55 gm
Qusetion 4
Balanced equation:
N2 + 3 H2 ====> 2 NH3
Reaction type: synthesis
650.0 grams of hydrogen will react with nitrogen to give 3660.87 gm of NH3
percent yield of this reaction = 1575 x 100 / 3660.87 = 43.02 %
Question 5
Balanced equation:
Fe2S3 + 4 O2 ====> 2 FeO + 3 SO2
Reaction type: double replacement
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