Question

For each unbalanced equation below, calculate how many grams of each product would be produced by complete reaction of 12.5g of the reactant indicated. Indicate clearly the mole ratio used for the conversion.
A. TiBr4(g)+H2(g)=Ti(s)+HBr(g), Reactant is H2
B. SiH4(g)+NH3(g)=Si3N4(s)+H2(g), Reactant is SiH4
C. NO(g)+H2(g)=N2(g)+2H2O(l), Reactant is H2
D. Cu2S(s)=Cu(s)+S(g), Reactant is Cu2S

Answer 1

These are stoichiometry problems.
1. Balance the equations.
2. Convert 12.5 g of the reactant indicated to mols. mols = grams/molar mass.
3. Using the coefficients in the balanced equation, convert mols of what you have to mols of what you want.
4. Convert mols of the product to grams.
Post your work if you get stuck. Explain fully what you don't understand.

Answer 2

B) = 3SiH4(g) + 4NH3(g)= SiN4(g) + 12N2
3: 1: 12= ratio
3= 3.125
1= 1.042
12= 12.5