contestada

5. 1.00 mol HNO3 is treated with 4.47 g of magnesium. Calculate the number of moles of
HNO3 after all the metal has reacted. The unbalanced reaction is
HNO3 (aq) + Mg(s) + Mg(NO3)2 (aq) + H2(g)
a. 0.632 mol b. 0.184 mol c. 1.00 mol d. OM(all HNO3 used up)

Respuesta :

TheSection

Answer:

The balanced equation is:

2 HNO3 + Mg ---> Mg(NO3)2 + H2

From the equation, we can see that we need twice the moles of HNO3 than the moles of Mg

Moles of Mg:

Molar mass of Mg = 24 g/mol

Moles = Given mass / Molar Mass

Moles of Mg = 4.47 / 24 = 0.18 moles (approx)

Hence, 2(moles of Mg) = 0.36 moles of HNO3 will be consumed

Number of moles of HNO3 after the reaction is finished is the number of unreacted moles of HNO3

Unreacted moles of HNO3 = Total Moles - Moles consumed

Unreacted moles of HNO3 = 0.64 moles (approx)

Since we approximated the value of moles of Mg, the value of remaining moles of HNO3 will also be approximate

From the given options, we can see that 0.632 moles is the closest value to our answer

Therefore, 0.632 moles will remain after the reaction

Otras preguntas