Question

According to the balanced reaction below, calculate the moles of NH3 that form when 4.2 mol of N2H4 completely reacts 3 N2H4(1) ► 4 NH3(g) + N2(g) Attempts remaining: 2 According to the balanced reaction below, calculate the moles of NO2 that form when 5.20 x 10-3 mol of N205 completely reacts: 2 N2O5(g) → 4 NO2(g) + O2(g) Attempts remaining: 2 How many moles of H2SO4 are required to completely react with 7.20 mol of Al according to the balanced chemical reaction: 2Al(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + 3 H2(g) Attempts remaining: 2 Determine the number of grams of C4H10 that are required to completely react to produce 8.70 mol of CO2 according to the following combustion reaction: 2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(g) 4

Answer 1

1)

From balanced equation,

Mol of NH3 formed = (4/3)*mol of N2H4 reacted

= (4/3)*4.2 mol

= 5.6 mol

Answer: 5.6 mol

2)

From balanced equation,

Mol of NO2 formed = (4/2)*mol of N2O5 reacted

= (4/2)*(5.20*10^-3) mol

= 0.0104 mol

Answer: 0.0104 mol

3)

From balanced equation,

Mol of H2SO4 required = (3/2)*mol of Al reacted

= (3/2)*7.20 mol

= 10.8 mol

Answer: 10.8 mol

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