How much heat is absorbed/released when 35.00 g of nh3(g) reacts in the presence of excess o2(g) to produce no(g) and h2o(l) according to the following chemical equation? 4 nh3(g) + 5 o2(g) → 4 no(g) + 6 h2o(l) h° = 1168 kj

Amount of energy absorbed = 600.06 kJ

Explanation:

Moles of :-

Mass = 35.00 g

Molar mass of = 17.031 g/mol

The formula for the calculation of moles is shown below:

Thus,

According to the reaction:-

Since, enthalpy change is positive, the heat is being absorbed.

4 moles of ammonia on reaction absorbs 1168 kJ of energy

1 mole of ammonia on reaction absorbs 1168/4 kJ of energy

So,

2.055 mole of ammonia on reaction absorbs (1168/4)*2.055 kJ of energy

Amount of energy absorbed = 600.06 kJ

your parents i think this could be it

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.