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Tpy6a [65]
2 years ago
10

How many mol of C3H8 are consumed when 3 mol of CO2 are produced ?

Chemistry
1 answer:
ser-zykov [4K]2 years ago
7 0

Answer:

1 mol C₃H₈

Explanation:

Step 1: Write the balanced equation for the combustion of C₃H₈

C₃H₈ + 5 O₂ ⇒ 3 CO₂ + 4 H₂O

Step 2: Establish the appropriate molar ratio

According to the balanced equation, the molar ratio of C₃H₈ to CO₂ is 1:3.

Step 3: Calculate the moles of C₃H₈ consumed when 3 moles of CO₂ are produced

We will use the established molar ratio.

3 mol CO₂ × 1 mol C₃H₈/3 mol CO₂ = 1 mol C₃H₈

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A 100-watt light bulb radiates energy at a rate of 100 J/s. (The watt, a unit of power or energy over time, is defined as 1 J/s.
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Answer

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Givens

  • Wavelength = λ = 525 * 10^-9 meters  [1 nmeter = 1*10^-9 meters]
  • c = 3 * 10^8 meters
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Formula

E = h * c / λ

W = E / t

Solution

E = 6.26 * 10^-34 j*s * 3 * 10^8 m/s /525 * 10^-9 (m)

The meters cancel out. So do the seconds. You are left with Joules as you should be.

E =  3.577 * 10^-18 Joules

What you have found is the energy of 1 photon.

Now you have to find the Joules from the watts.

W = E/t

100 * 1 second = 100 joules

1 photon contains 3.577 * 10 ^ - 18 Joules

x photon = 100 joules                        

1/x = 3.577 * 10^-18 / 100                          Cross multiply

100 = 3.577 * 10 ^ - 18 * x                         Divide both sides by 3.577 * 10 ^ - 18

100/3.577 * 10 ^ - 18 = 3.577 * 10 ^ - 18x / 3.577 * 10 ^ - 18

2.7956 * 10^19 photons = x


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