For the reaction shown, calculate how many moles of NO 2 form when each amount of reactant completely reacts. 2N 2 O 5 (g)→4NO 2 (g)+O 2 (g)

2.0mol N 2 O 5
6.4mol N 2 O 5
10.0g N 2 O 5
1.50kg N 2 O 5

For each reaction, calculate the mass (in grams) of the product formed when 10.1g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

2K(s)+Cl 2 (g) - - - - - →2KCl(s)
2K(s)+Br 2 (l) - - - - - →2KBr(s)
4Cr(s)+3O 2 (g) - - - - - →2Cr 2 O 3 (s)
2Sr(s) - - - - +O 2 (g)→2SrO(s)

What is the concentration of K + in 0.15 M of K 2 S ?
A scientist wants to make a solution of tribasic sodium phosphate, Na 3 PO 4 , for a laboratory experiment. How many grams of Na 3 PO 4 will be needed to produce 275mL of a solution that has a concentration of Na + ions of 1.40M ?