How much water would form if 2.56 g of hydrogen reacted completely with 20.32 g of oxygen?

2 H2 + O2 → 2 H2O

(2.56 g H2) / (2.01588 g H2/mol) = 1.2699 mol H2

(20.32 g O2) / (31.99886 g O2/mol) = 0.6350226 mol O2

1.2699 moles of H2 would react completely with 1.2699 x (1/2) = 0.63495 mole of O2, but there is very slightly more O2 present than that, so O2 is in small excess and H2 is barely

hope this helps

prolly a beacuse the momentuem the car has increases while going down hill

the old price per ounce is c/4.

the new price per ounce is c/3.6.

the ratio of the old price to the new one is

(c/4)/(c/3.6) = (c/c)×(3.6/4) = 0.9 . . = 9/10 . . "nine tenths" in either form