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seraphim [82]
3 years ago
5

The combustion of 1.38 grams of a compound which contains C, H, O and N yields 1.72 grams of CO2 and 1.18 grams of H2O. Another

sample of the compound with a mass of 22.34 grams is found to contain 6.75 grams of O. What is the empirical formula of the compound?
Chemistry
1 answer:
I am Lyosha [343]3 years ago
6 0

Answer:

The empirical formula is C3H10N2O2

Explanation:

Step 1: Data given

Mass of the sample in experiment 1 = 1.38 grams

Mass of CO2 produced = 1.72 grams

Mass of H2O produced = 1.18 grams

Molar mass CO2 = 44.01 g/mol

Molar mass H2O = 18.02 g/mol

Atomic mass C = 12.01 g/mol

Atomic mass O = 16.0 g/mol

Atomic mass H = 1.01 g/mol

MAss of the sample in experiment 2 = 22.34 grams

Mass of O = 6.75 grams

Step 2: Calculate moles CO2

Moles CO2 = mass CO2 / molar mass CO2

Moles CO2 = 1.72 grams / 44.01 g/mol

Moles CO2 = 0.0391 moles

Step 3: Calculate moles C

For 1 mol CO2 we have 1 mol C

For 0.0391 moles CO2 we have 0.0391 moles C

Step 4: Calculate mass C

Mass C = 0.0391 moles * 12.01 g/mol

Mass C = 0.470 grams

Step 5: Calculate moles H2O

Moles H2O = 1.18 grams / 18.02 g/mol

Moles H2O = 0.0655 moles

Step 6: Calculate moles H

For 1 mol H2O we have 2 moles H

For 0.0655 moles H we have 2*0.0655 = 0.131 moles H

Step 7: Calculate mass H

Mass H = 0.131 moles * 1.01 g/mol

Mass H = 0.132 grams

Step 8: Calculate the mass %

% C = (0.470 grams / 1.38 grams) * 100 %

% C = 34.06 %

%H = (0.132/1.38)*100 %

%H = 9.57 %

%O= (6.75 grams / 22.34 grams)*100 %

%O = 30.21 %

%N = 100 % - 34.06 % - 9.57 % - 30.21 %

%N = 26.16 %

Step 8: Calculate moles in compound

Let's assume 100 grams sample then we have:

Mass C = 34.06 grams

Mass H = 9.57 grams

Mass O = 30.21 grams

Mass N = 26.16 grams

Moles C= 34.06 grams / 12.01 g/mol

Moles C= 2.836 moles

Moles H = 9.57 grams / 1.01 g/mol

Moles H = 9.475 moles

Moles O = 30.21 grams / 16.0 g/mol

Moles O = 1.888 moles

Moles N = 26.16 grams / 14.0 g/mol

Moles N = 1.869 moles

Step 9: Calculate mol ratio

We have to divide by the smallest amount of moles

C: 2.836 moles / 1.869 moles = 1.5

H: 9.475 moles /1.869 moles = 5

O: 1.888 moles /1.869 moles = 1

N: 1.869 moles / 1.869 moles = 1

This means for each mol O we have 1.5 moles C, 5 moles H and 1 mol N

OR

For every 2 O atoms we have 3 C atoms, 10 H atoms and 2 N atoms

The empirical formula is C3H10N2O2

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4 0
3 years ago
A 60.0 g block of iron that has an initial temperature of 250. °C and 60.0 g bloc of gold that has an initial temperature of 45.
Maslowich

Answer:

The final temperature at the equilibrium is 204.6 °C

Explanation:

Step 1: Data given

Mass of iron = 60.0 grams

Initial temperature = 250 °C

Mass of gold = 60.0 grams

Initial temperature of gold = 45.0 °C

The specific heat capacity of iron = 0.449 J/g•°C

The specific heat capacity of gold = 0.128 J/g•°C.

Step 2: Calculate the final temperature at the equilibrium

Heat lost = Heat gained

Qlost = -Qgained

Qiron = -Qgold

Q=m*c*ΔT

m(iron) * c(iron) *ΔT(iron) = -m(gold) * c(gold) *ΔT(gold)

⇒with m(iron) = the mass of iron = 60.0 grams

⇒with c(iron) = the specific heat of iron = 0.449 J/g°C

⇒with ΔT(iron)= the change of temperature of iron = T2 - T1 = T2 - 250.0°C

⇒with m(gold) = the mass of gold= 60.0 grams

⇒with c(gold) = the specific heat of gold = 0.128 J/g°C

⇒with ΔT(gold) = the change of temperature of gold = T2 - 45.0 °C

60.0 *0.449 * (T2 - 250.0) = -60.0 * 0.128 * (T2 - 45.0 )

26.94 * (T2 - 250.0) = -7.68 * (T2 - 45.0)

26.94T2 - 6735 = -7.68T2 + 345.6

34.62T2 = 7080.6

T2 = 204.5 °C

The final temperature at the equilibrium is 204.6 °C

5 0
3 years ago
What is the mole ratio of H2O to C8H8?
zepelin [54]

Answer:

Mole ratio for a compound

The chemical formula tells us the mole ratio.

CO2 = 1 CO2 molecule : 1 C atom : 2 O atoms.

Mole ratio for a reaction

The balanced chemical reactions tells us.

C12H22O11 + 12 O2  12 CO2 + 11 H2O

1 C12H22O11 molecule: 12 O2 molecules : 12 CO2

molecules : 11 H2O molecules.

Applications of the mole ratio concept

grams <--> moles <--> moles <--> grams

Explanation:

4 0
3 years ago
Samuel adds a teaspoon of salt to a glass of water. He notices that the salt disappears. Samuel takes a sip to discover that the
Vera_Pavlovna [14]

Answer:

B

Explanation:

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4 0
3 years ago
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How many grams are in 5 moles of 7.75 grams?
lesya692 [45]

Answer:

21

Explanation:

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5 0
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