Question

Сколько граммов пятнадцатипроцентной H2SO4 необходимо для растворения 9,6 граммов Fe2O3 ?

Answer 1

 Xg             9.6 g
3H2SO4+Fe2O3-->3H2O+Fe2(SO4)3
 3*98              160                               
M(H2SO4)=98 g/mol  M(Fe2O3)=160 g/mol
x/294 = 9.6 / 160
X=17.64 g
m(ppa)=17.64*100%/15%=117.6g
ответ 117.6 г

Answer 2

У меня там ошибка не246,а 294
так что 100%-17.64
15%-2,6

Answer 3

Calculating the Amount of 15% H2SO4 Needed to Dissolve 9.6 grams of Fe2O3

To calculate the amount of 15% H2SO4 needed to dissolve 9.6 grams of Fe2O3, we can use the chemical equation for the reaction between Fe2O3 and H2SO4. The balanced chemical equation for the reaction is:

Fe2O3 + H2SO4 → Fe2(SO4)3 + H2O

From the balanced chemical equation, we can see that 1 mole of Fe2O3 reacts with 3 moles of H2SO4. We can use this information to calculate the amount of 15% H2SO4 needed to dissolve 9.6 grams of Fe2O3.

First, we need to calculate the moles of Fe2O3: - The molar mass of Fe2O3 is approximately 159.69 g/mol. - Therefore, the moles of Fe2O3 can be calculated as: moles = mass / molar mass moles = 9.6 g / 159.69 g/mol

Next, we can use the mole ratio from the balanced chemical equation to calculate the moles of H2SO4 needed: - According to the balanced chemical equation, 1 mole of Fe2O3 reacts with 3 moles of H2SO4.

Finally, we can convert the moles of H2SO4 to grams of 15% H2SO4 solution using the concentration of the solution.

Let's calculate the amount of 15% H2SO4 needed to dissolve 9.6 grams of Fe2O3.

Calculation:

- Moles of Fe2O3: moles = 9.6 g / 159.69 g/mol

- Moles of H2SO4 needed: moles of H2SO4 = moles of Fe2O3 * (3 moles of H2SO4 / 1 mole of Fe2O3)

- Grams of 15% H2SO4 solution needed: grams = moles of H2SO4 * molar mass of H2SO4 * (100 / 15)

Let's calculate the values based on the given information.

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