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Nikolay [14]
3 years ago
15

How much heat is released when 6.00 g of methane is combusted using the reaction below? CH4 + 2O2 ? CO2 + 2H2O ?Hrxn = -890. KJ

Chemistry
2 answers:
goblinko [34]3 years ago
8 0

Answer : The amount of heat released is, -121.04 KJ

Solution : Given,

Enthalpy of reaction, \Delta H_{rxn} = -890 KJ

Mass of methane = 6 g

Molar mass of methane = 44 g/mole

First we have to calculate the moles of methane.

\text{Moles of methane}=\frac{\text{Mass of methane}}{\text{Molar mass of methane}}=\frac{6g}{44g/mole}=0.136moles

The given balanced reaction is,

CH_4+2O_2\rightarrow CO_2+2H_2O

From the balanced reaction we conclude that

1 mole of methane releases heat = -890 KJ

0.136 moles of methane releases heat = \frac{0.136moles}{1mole}\times -890KJ=-121.04KJ

Therefore, the amount of heat released is, -121.04 KJ

anastassius [24]3 years ago
3 0

Answer:

-333.75 KJ

Explanation:

From the reaction CH₄ + 2O₂ ⇒ CO₂ + 2H₂O    ΔHrxn = -890 KJ.

From the reaction, 1 mole of CH₄ combusts to give -890 KJ.

We now calculate the number of moles, n of CH₄ in 6.00g

n = mass of CH₄/molar mass of CH₄

molar mass of CH₄ = 12 g/mol + 4 × 1 g/mol = (12 + 4) g/mol = 16 g/mol

mass of CH₄ = 6.00 g

n = 6.00 g /16 g/mol = 0.375 mol

So we have 0.375 mol of CH₄ in 6.00g

From the reaction, 1 mole of CH₄ produces -890 KJ

then 0.375 mol produces 0.375 mol × -890 KJ/1 mol = -333.75 KJ

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Help please with question number 16)
Zanzabum

Answer:

Mg²⁵   =   10.00%    

Mg²⁶   =   45.04%

Mg²⁴   =   44.96%

Explanation:

Given data:

Atomic mass of Mg²⁶ = 25.983

Atomic mass of Mg²⁵ = 24.986

Atomic mass of Mg²⁴ = 23.985

Abundance of Mg²⁵ = 10.00%

Abundance of Mg²⁶ = ?

Abundance of Mg²⁴ = ?

Solution:

Average atomic weight of Mg = 25.983  + 24.986+ 23.985 / 3

Average atomic weight of Mg = 74.954/3

Average atomic weight of Mg = 24.985 amu

Abundance of          

Mg²⁵   =   10.00    

Mg²⁶   =    x      

Mg²⁴   =   100- 10 - x = 90 -x    

Formula:

Average atomic mass  = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass) + (abundance of 3rd isotope × its atomic mass)  / 100

24.985 = (0.1×24.986)+(90-x×23.985) + ( x ×25.983 )  /100

24.985 =  249.86 + 2158.65 - 23.985x + 25.983x  / 100

24.985 = 2408.51 + 1.998 x / 100

2498.5 = 2408.51 + 1.998 x

1.998 x = 2498.5 - 2408.51

1.998 x = 89.99

x = 89.99 /1.998

x = 45.04

Now we put the value of x:

Mg²⁵   =   10.00    

Mg²⁶   =    x  (45.04)

Mg²⁴   =   90 -x   (90 - 45.04 = 44.96)

5 0
2 years ago
A student reacts 20.0 mL of 0.248 M H2SO4 with 15.0 mL of 0.195 M NaOH. Write a balanced chemical equation to show this reaction
Molodets [167]

<u>Answer:</u> The concentration of salt (sodium sulfate), sulfuric acid and NaOH in the solution is 0.0418 M, 0.0999 M and 0 M respectively.

<u>Explanation:</u>

To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}     .....(1)

<u>For NaOH:</u>

Initial molarity of NaOH solution = 0.195 M

Volume of solution = 15.0 mL = 0.015 L   (Conversion factor:   1 L = 1000 mL)

Putting values in equation 1, we get:

0.195M=\frac{\text{Moles of NaOH}}{0.015L}\\\\\text{Moles of NaOH}=(0.195mol/L\times 0.015L)=2.925\times 10^{-3}mol

<u>For sulfuric acid:</u>

Initial molarity of sulfuric acid solution = 0.248 M

Volume of solution = 20.0 mL = 0.020 L

Putting values in equation 1, we get:

0.248M=\frac{\text{Moles of }H_2SO_4}{0.020L}\\\\\text{Moles of }H_2SO_4=(0.248mol/L\times 0.020L)=4.96\times 10^{-3}mol

The chemical equation for the reaction of NaOH and sulfuric acid follows:

2NaOH+H_2SO_4\rightarrow Na_2SO_4+2H_2O

By Stoichiometry of the reaction:

2 moles of NaOH reacts with 1 mole of sulfuric acid

So, 2.925\times 10^{-3} moles of KOH will react with = \frac{1}{2}\times 2.925\times 10^{-3}=1.462\times 10^{-3}mol of sulfuric acid

As, given amount of sulfuric acid is more than the required amount. So, it is considered as an excess reagent.

Thus, NaOH is considered as a limiting reagent because it limits the formation of product.

Excess moles of sulfuric acid = (4.96-1.462)\times 10^{-3}=3.498\times 10^{-3}mol

By Stoichiometry of the reaction:

2 moles of KOH produces 1 mole of sodium sulfate

So, 2.925\times 10^{-3} moles of KOH will produce = \frac{1}{2}\times 2.925\times 10^{-3}=1.462\times 10^{-3}mol of sodium sulfate

  • <u>For sodium sulfate:</u>

Moles of sodium sulfate = 1.462\times 10^{-3}moles

Volume of solution = [15.0 + 20.0] = 35.0 mL = 0.035 L

Putting values in equation 1, we get:

\text{Molarity of sodium sulfate}=\frac{1.462\times 10^{-3}}{0.035}=0.0418M

  • <u>For sulfuric acid:</u>

Moles of excess sulfuric acid = 3.498\times 10^{-3}mol

Volume of solution = [15.0 + 20.0] = 35.0 mL = 0.035 L

Putting values in equation 1, we get:

\text{Molarity of sulfuric acid}=\frac{3.498\times 10^{-3}}{0.035}=0.0999M

  • <u>For NaOH:</u>

Moles of NaOH remained = 0 moles

Volume of solution = [15.0 + 20.0] = 35.0 mL = 0.035 L

Putting values in equation 1, we get:

\text{Molarity of NaOH}=\frac{0}{0.050}=0M

Hence, the concentration of salt (sodium sulfate), sulfuric acid and NaOH in the solution is 0.0418 M, 0.0999 M and 0 M respectively.

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Answer:

True

Explanation:

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