In the reaction of aluminum and iron(iii) oxide to form iron and aluminum oxide, δh is -850 kj. how many grams of aluminum oxide are formed when 350 kj of heat are released? 2 al (s) + fe2o3 (s) → 2 fe (s) + al2o3 (s) δh= -850 kj

When 350 kJ are released there are formed 41,98 g of aluminium oxide.

Explanation:

For the reaction:

2Al (s) + Fe₂O₃ (s) → 2Fe (s) + Al₂O₃(s)

There are produced 850 kJ.

350 kJ of energy produced are when are formed:

350 kJ × = 0,412 moles of Aluminium oxide.

As molar mass of aluminium oxide is 101,96 g/mol. The grams in 0,412 moles of Al₂O₃ are:

0,412 moles Al_{2}O_{3} × = 41,98 g

Thus, when 350 kJ are released there are formed 41,98 g of aluminium oxide.

I hope it helps!

the answer is true.

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.