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miskamm [114]
3 years ago
9

The following reaction shows the products when sulfuric acid and aluminum hydroxide react.

Chemistry
1 answer:
SSSSS [86.1K]3 years ago
6 0

Answer:

There will remain 11.47 grams of Al(OH)3

Explanation:

Step 1: Data given

Mass of sulfuric acid = 35.0 grams

Molar mass sulfuric acid = 98.08 g/mol

Mass of aluminium hydroxide = 30.0 grams

Molar mass of aluminium hydroxide = 78.0 g/mol

Step 2: The balanced equation

2Al(OH)3 + 3H2SO4 → Al2(SO4)3 + 6H2O

Step 3: Calculate moles

Moles = mass / molar mass

Moles Al(OH)3 = 30.0 grams / 78.0 g/mol

Moles Al(OH)3 = 0.385 moles

Moles H2SO4 = 35.0 grams / 98.08 g/mol

Moles H2SO4 = 0.357 moles

Step 4: Calculate the limiting reactant

For 2 moles Al(OH)3 we need 3 moles H2SO4 to produce 1 mol Al(SO4)3 and 6 moles H20

H2SO4 is the limiting reactant. It will completely be consumed ( 0.357 moles). Al(OH)3 is in excess. There will be react 2/3 * 0.357 = 0.238 moles

There will remain 0.385 - 0.238 = 0.147 moles

Mass of Al(OH)3 remaining = 0.147 moles* 78.0 g/mol = 11.47 grams

There will remain 11.47 grams of Al(OH)3

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C – 19,9%, H – 2,2%, N – 11,6%, O – x%

M=120\frac{g}{mol}

1 percentage

The entire molecule is 100% and all the components of the compound add up to 100%.

100% - 19,9% - 2,5% - 11,6% = 66,1%

The compound contains 66,1% oxygen.

2 molar masses

M_{C}=12,01\frac{g}{mol}

M_{H}=1,008\frac{g}{mol}

M_{O}=15,999\frac{g}{mol}

M_{N}=14,007\frac{g}{mol}

3 masses

The compound has a molar mass of 120g/mol. So one molecule weighs 120 g. To find out how much the percentage of a component weighs, you have to calculate it using the molar mass.

<u>carbon</u>

19,8% of 120g

m=120g*0,198\\m=23,76g

One molecule contains 23,76g of carbon.

<u>hydrogen</u>

2,5% of 120g

m=120g*0,025\\m=3g

One molecule contains 3g of hydrogen.

<u>oxygen</u>

66,1% of 120g

m=120g*0,661\\m=79,32g

One molecule contains 79,32g of oxygen.

<u>nitrogen</u>

11,6% of 120g

m=120g*0,0,116\\m=13,92g

One molecule contains 13,92g of nitrogen.

4 amount of substance

<u>carbon</u>

<u />n=\frac{23,76g}{12,01\frac{g}{mol} }\\n=1,98mol<u />

The compound contains about 2 moles of carbon.

<u>hydrogen</u>

n=\frac{3g}{1\frac{g}{mol} }\\n=3mol

The compound contains about 3 moles of hydrogen.

<u>oxygen</u>

n=\frac{79,32g}{15,999\frac{g}{mol} }\\n=4,96mol

The compound contains about 5 moles of oxygen.

<u>nitrogen</u>

<u />n=\frac{13,92g}{14,007\frac{g}{mol} }\\n=0,99mol<u />

The compound contains about 1 moles of nitrogen.

5. molecular formula

The formula results from the ratio of the amounts of substance.

n_{C} :n_{H} :n_{O} :n_{N} =2:3:5:1\\C_{2}H_{3}NO_{5}

8 0
3 years ago
How many milliliters of a 1.25 molar HCL solution would be needed to react completely with 60 g of calcium metal
Svet_ta [14]
Ca + 2HCl = CaCl₂ + H₂

m(Ca)=60 g
c=1.25 mol/l
M(Ca)=40g/mol
v-?

m(Ca)/M(Ca)=m(HCl)/[2M(HCl)]=n(HCl)/2

n(HCl)=2m(Ca)/M(Ca)

n(HCl)=cv

cv=2m(Ca)/M(Ca)

v=2m(Ca)/{cM(Ca)}

v=2·60g/mol/{1.25mol/l·40g/mol}=2.4 l = 2400 ml

2400 milliliters of a 1.25 molar HCl solution would be needed

3 0
3 years ago
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valentina_108 [34]
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What is the mass in grams of 9.45*10^24 molecules of methanol (CH3OH)?
Angelina_Jolie [31]
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1 mole ---------- 6.02x10²³ molecules
? moles --------- 9.45x10²⁴ molecules

1 x ( 9.45x10²⁴) / 6.02x10²³ =

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Therefore:

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Mass methanol  = 15.69 x 32.04 / 1 => 502.7076 g


6 0
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