3Ag(s) + 4HNO3(AQ) = 3AGNO3(aq) + NO(g) + 2h2o(l)
How many moles of NO can be produced by the reaction of 54.0g of Ag
show me the step please
mols Ag = grams/molar mass = ?
The coefficients tell you exactly how much NO you get. You get 1 mol NO for every 3 mols Ag; therefore,
mols NO = ?mols Ag x (1 mol NO/3 mol Ag) = ?mols x (1/3) = xx mol NO.
To find the moles of NO produced by the reaction, you will need to use the balanced chemical equation and the molar mass of Ag. Here are the steps to calculate it:
Step 1: Write and balance the chemical equation.
The balanced equation for the reaction is:
3Ag(s) + 4HNO3(aq) → 3AgNO3(aq) + NO(g) + 2H2O(l)
Step 2: Determine the molar mass of Ag.
The molar mass of Ag is 107.87 g/mol. You can find this value on the periodic table.
Step 3: Convert the given mass of Ag to moles.
To do this, divide the given mass (54.0 g) by the molar mass of Ag:
54.0 g Ag × (1 mol Ag / 107.87 g Ag) = 0.500 mol Ag
Step 4: Use the stoichiometry of the balanced equation to find the moles of NO.
From the balanced equation, you can see that the stoichiometric ratio between Ag and NO is 3:1. This means that for every 3 moles of Ag reacted, 1 mole of NO is produced.
Therefore, the moles of NO can be calculated as:
0.500 mol Ag × (1 mol NO / 3 mol Ag) = 0.167 mol NO
Thus, the reaction of 54.0 g of Ag will produce 0.167 moles of NO.