Astudent determines the aluminum content of a solution by first precipitating it as aluminum hydroxide, and then decomposing the hydroxide to aluminum oxide by heating. how many grams of aluminum oxide should the student obtain if her solution contains 40.0 ml of 0.541 m aluminum nitrate?

The student should obtain 1.103 g of aluminum oxide

Explanation:

Al(NO3)3 + 3NaOH → 3NaNO3 + Al(OH)3

Now,  the equation that represents the decomposition of the hydroxide to aluminum oxide by heating it.

2Al(OH)3 → Al2O3 + 3H2O

Volumen of  Al(NO3)3 = 40mL

Molar concentration of Al(NO3)3 =  0.541M

Molecular Weight Al2O3 = 101.96 g/mol

then we use the molar coefficients from the  equations to discover the amount of Al2O3  moles produced

finally, we use the molecular weight of the Al2O3  to calculate the final mass produced.

plants need sunlight, water, and carbon dioxide to make food. plants use the raw materials of water, nutrients they absorb from soil, and carbon dioxide to make sugars the plant can use. energy from the sun and chlorophyll are also needed.

answer: they produce more slow than unicellular organisms.