I just have three questions that are causing me a few troubles.
Showing your work can greatly help me out.
(I have worked out the chemical equations. If some are wrong, don't hesitate to correct me!)
The reaction of Ammonia and Sulfuric Acid to form Ammonium Sulfate is used in the commercial production of fertilizer.
a) Write the balanced chemical equation: 2 NH3 + H2SO4 -> (NH4)2SO4
b) If 22.7 grams Ammonia and 54.8 grams Sulfuric Acid are allowed to react, how many grams of Ammonium Sulfate can be formed? Identify the limiting reactant.
2. Determine the empirical formula of a compound that is 54.53% Carbon, 9.15% Hydrogen, and 36.32% Oxygen.
a) (I have found the empirical formula to be C2H4O.)
b) What is the molecular formula of the compound if its molecular mass is 88 amu?
3. Nitric Acid decomposes to form aqueous Nitrogen Dioxide, Water, and a gas, which relights a glowing splint.
a) Write a balanced chemical equation: 4 HNO3 -> 4 NO2 + 2 H2O + O2
b) If 6.5 moles of Nitrogen Dioxide is produced, what mass, in grams, of Nitric Acid reacted?
If you don't wish to do the problem, just show the work! I'll be able to figure out the answer with little explanation.
Showing your work can greatly help me out.
(I have worked out the chemical equations. If some are wrong, don't hesitate to correct me!)
The reaction of Ammonia and Sulfuric Acid to form Ammonium Sulfate is used in the commercial production of fertilizer.
a) Write the balanced chemical equation: 2 NH3 + H2SO4 -> (NH4)2SO4
b) If 22.7 grams Ammonia and 54.8 grams Sulfuric Acid are allowed to react, how many grams of Ammonium Sulfate can be formed? Identify the limiting reactant.
2. Determine the empirical formula of a compound that is 54.53% Carbon, 9.15% Hydrogen, and 36.32% Oxygen.
a) (I have found the empirical formula to be C2H4O.)
b) What is the molecular formula of the compound if its molecular mass is 88 amu?
3. Nitric Acid decomposes to form aqueous Nitrogen Dioxide, Water, and a gas, which relights a glowing splint.
a) Write a balanced chemical equation: 4 HNO3 -> 4 NO2 + 2 H2O + O2
b) If 6.5 moles of Nitrogen Dioxide is produced, what mass, in grams, of Nitric Acid reacted?
If you don't wish to do the problem, just show the work! I'll be able to figure out the answer with little explanation.
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Hello,
1 a) Is correct
b) Utilize the equation as a reference:
22.7g NH3 x (1 mole NH3/ 17.034g NH3) x (1 mole H2SO4/ 2 mole NH3) x (98.076g H2SO4/ 1 mole H2SO4) = 65.35g H2SO4 that can react completely with 22.7g NH3. Since we are only given 54.8g H2SO4, we are lacking in H2SO4 thus it is the Limiting Reactant. Now we will use the LR to solve the rest of the problem.
54.8g H2SO4 x (1 mole H2SO4/ 98.076g H2SO4) x (1 mole (NH4)2SO4/ 1 mole H2SO4) x (132.144g (NH4)2SO4/ 1 mole (NH4)2SO4) = 73.0 grams of (NH4)2SO4 can be produced.
2 a) Is correct
b) Since we've found the "empirical" formula, let's find its mass and create a ratio with the "molecular" formula's mass. Thus..
1 a) Is correct
b) Utilize the equation as a reference:
22.7g NH3 x (1 mole NH3/ 17.034g NH3) x (1 mole H2SO4/ 2 mole NH3) x (98.076g H2SO4/ 1 mole H2SO4) = 65.35g H2SO4 that can react completely with 22.7g NH3. Since we are only given 54.8g H2SO4, we are lacking in H2SO4 thus it is the Limiting Reactant. Now we will use the LR to solve the rest of the problem.
54.8g H2SO4 x (1 mole H2SO4/ 98.076g H2SO4) x (1 mole (NH4)2SO4/ 1 mole H2SO4) x (132.144g (NH4)2SO4/ 1 mole (NH4)2SO4) = 73.0 grams of (NH4)2SO4 can be produced.
2 a) Is correct
b) Since we've found the "empirical" formula, let's find its mass and create a ratio with the "molecular" formula's mass. Thus..
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