Question 4-6 refer to : 3Ag(s) + 4HNO3(AQ) = 3AGNO3(aq) + NO(g) + 2h2o(l)
4. How many moles of NO can be produced by the reaction of 54.0g of Ag?
5. How many grams of AgNO3 can be produced by recating completely 88.0g of Ag?
6. State the number of grams of water that can be obtained by the reaction of 324g of Ag with 126g of HNO3?
I have given this link to you before. Just follow the steps in this worked example.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To answer these questions, we need to use the given balanced chemical equation and the concept of stoichiometry.
The balanced chemical equation is:
3Ag(s) + 4HNO3(aq) = 3AgNO3(aq) + NO(g) + 2H2O(l)
4. To find the number of moles of NO produced, we first need to calculate the number of moles of Ag. To do this, we need to use the molar mass of Ag, which is 107.87 g/mol.
Number of moles of Ag = Mass of Ag / Molar mass of Ag
Number of moles of Ag = 54.0 g / 107.87 g/mol
Now, using the balanced chemical equation, we can relate the number of moles of Ag to the number of moles of NO. From the balanced equation, we see that 3 moles of Ag produce 1 mole of NO.
Number of moles of NO = (Number of moles of Ag) × (1 mole of NO / 3 moles of Ag)
5. To find the number of grams of AgNO3 produced, we need to first calculate the number of moles of Ag using the same formula as in question 4.
Number of moles of Ag = 88.0 g / 107.87 g/mol
Now using the balanced chemical equation, we can relate the number of moles of Ag to the number of moles of AgNO3. From the balanced equation, we see that 3 moles of Ag produce 3 moles of AgNO3.
Number of moles of AgNO3 = (Number of moles of Ag) × (3 moles of AgNO3 / 3 moles of Ag)
6. To find the number of grams of H2O produced, we first need to calculate the number of moles of Ag and HNO3. Then we can use the balanced chemical equation to relate the number of moles of Ag and HNO3 to the number of moles of H2O. Finally, we can convert the number of moles of H2O to grams using the molar mass of water (H2O), which is 18.02 g/mol.
Number of moles of Ag = 324 g / 107.87 g/mol
Number of moles of HNO3 = 126 g / (1 g/mol (since HNO3 is already in molar form))
Now using the balanced chemical equation, we can relate the number of moles of Ag and HNO3 to the number of moles of H2O. From the balanced equation, we see that 2 moles of H2O can be produced from 3 moles of Ag and 4 moles of HNO3.
Number of moles of H2O = min(Number of moles of Ag × (2 moles of H2O / 3 moles of Ag),
Number of moles of HNO3 × (2 moles of H2O / 4 moles of HNO3))
To get the grams of H2O, simply multiply the number of moles of H2O by the molar mass of water:
Mass of H2O = Number of moles of H2O × Molar mass of H2O
I hope this explanation helps you understand how to solve these types of stoichiometry problems!