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Mazyrski [523]
2 years ago
5

the bunsen burners in your labs are fueled by natural gas which is mostly methane. the thermochemical equation for the combustio

n of methane is
Chemistry
1 answer:
vampirchik [111]2 years ago
5 0

Answer:

CH₄ + 2O₂ —> CO₂ + 2H₂O

Explanation:

The thermochemical equation for the combustion of methane can be obtained as follow:

Methane (CH₄) under goes combustion in the presence of air (O₂) to produce carbon dioxide (CO₂) and water (H₂O). This can be represented in the equation below:

CH₄ + O₂ —> CO₂ + H₂O

Thus, we can balance the equation as follow:

CH₄ + O₂ —> CO₂ + H₂O

There are 4 atoms of H on the left side and 2 atoms on the right side. It can be balance by putting 2 in front of H₂O as shown below:

CH₄ + O₂ —> CO₂ + 2H₂O

There are a total of 4 atoms of O on the right side and 1 atom on the left side. It can be balance by putting 2 in front of O₂ as shown below:

CH₄ + 2O₂ —> CO₂ + 2H₂O

Now the equation is balanced.

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A gas occupies a volume of 1.00 L at 25.0°C. What volume will the gas occupy at 1.00 x10^2 °C?
Leno4ka [110]

Answer : The volume of gas occupy at 1.00\times 10^2^oC is, 1.25 L

Explanation :

Charles' Law : It states that volume of the gas is directly proportional to the temperature of the gas at constant pressure and number of moles.

Mathematically,

\frac{V_1}{T_1}=\frac{V_2}{T_2}

where,

V_1\text{ and }T_1 are the initial volume and temperature of the gas.

V_2\text{ and }T_2 are the final volume and temperature of the gas.

We are given:

V_1=1.00L\\T_1=25.0^oC=(25.0+273)K=298K\\V_2=?\\T_2=1.00\times 10^2^oC=((1.00\times 10^2)+273)K=373K

Putting values in above equation, we get:

\frac{1.00L}{298K}=\frac{V_2}{373K}\\\\V_2=1.25L

Therefore, the volume of gas occupy at 1.00\times 10^2^oC is, 1.25 L

3 0
3 years ago
What volume is occupied by 8.7 g of chlorine gas, Cl2, at 23°C and 1.15 atm pressure
Harrizon [31]

Answer:

V = 5.17L

Explanation:

Mass of gas = 8.7g

T = 23°C = (23 + 273.15)K = 296.15K

P = 1.15 atm

V = ?

R = 0.082atm.L / mol.K

From ideal gas equation

PV = nRT

P = pressure of the gas

V = volume of the gas

n = no. Of moles

R = ideal gas constant

T = temperature of the gas

no of moles = mass / molar mass

Molar mass of Chlorine = 35.5g / mol

No. Of moles = 8.7 / 35.5

No. Of moles = 0.245 moles

PV = nRT

V = nRT / P

V = (0.245 * 0.082 * 296.15) / 1.15

V = 5.9496 / 1.15

V = 5.17L

The volume of the gas is 5.17L

4 0
3 years ago
4. Which statement is true?
worty [1.4K]

Answer:

give a picture

Explanation:

4 0
3 years ago
Why does the density of a substance stay constant even if the mass of the substance increases?
olganol [36]

Answer:

If the mass stays constant the object's density decreases as the volume increases. ... Because the property of density is a constant for all variables, density can be used to identify the material an object is made of.

Explanation:

5 0
3 years ago
How many grams of NaCl are needed to prepare 50.0 grams of 35.0% of salt solution?
nevsk [136]

Answer:

17.5 g

Explanation:

Given data

  • Mass of solution to be prepared: 50.0 grams
  • Concentration of the salt solution: 35.0%

The concentration by mass of NaCl in the solution is 35.0%, that is, there are 35.0 grams of sodium chloride per 100 grams of solution. We will use this ratio to find the mass of sodium chloride required to prepare 50.0 grams of a 35.0% salt solution.

50.0gSolution \times \frac{35.0gNaCl}{100gSolution} = 17.5gNaCl

4 0
3 years ago
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