How many liters of NO are produced when 0.85 L of 2.00M HNO3 solution is added to 216g of Ag?whats limiting?

Question

GIVEN- 3Ag+4HNO3=3AgNO3+NO+2H20
whats limiting reactant

please help me.i dont know the steps in doing this.

Answer 1

216/107.868 = 2.00 moles Ag+

Moles HNO3 = 2.00(0.85)/1=1.7

The ratio between Ag+ and HNO3 is 3 : 4

3 : 4 = 2.00 : x
x= 2.67 moles HNO3 needed

We have only 1.7 moles HNO3 so it is the limiting reactant

The ratio between HNO3 and NO is 4 :1

4 : 1 = 1.7 : x

x = 0.425 moles NO produced

Liters produced

1 mole a STP has a volume =22.4 l

0.425 mole >>9.52 L

Answer 2

1) The reaction is:

3Ag+4HNO3 ---------> 3AgNO3+NO+2H20

2) First, we need to know how many moles there are of each species:

moles of HNO3 = (0.85 L)(2 moles/L) = 1.7 moles
moles of Ag = 216 g / 108g/mol = 2 moles

The balanced reaction shows that we need 3 moles of Ag and 4 moles of HNO3 to produce 3 moles of AgNO3 and 1 mol of NO (plus water). It means, Ag/HNO3 = 3/4 = 0.75

We can check the moles ratio of reactants:

Ag / HNO3 = 2 / 1.7 = 1.176

As 1.176 > 0.75 It means that all the HNO3 will be consumed before the silver. Hence the HNO3 is the limiting reactant.

3) To know how many liters of NO are produced we first compute number of moles we can get from 1.7 moles of HNO3 (because is the limiting reactant):

4 moles HNO3... ---- 1 mol NO
1.7 moles HNO3 ---- x

x= 0.425 moles

Knowing that 1 mol of a gas substance occupies 22.4 liters in STP conditions, the volume of produced NO is:

V = (22.4 L)(0.425 moles) = 9.52 Liters

That's it!

Good luck!