This problem asks us to calculate the number of photons emitted per second by a bulb, given its power rating, light conversion efficiency, and the energy of a single photon.
First, we determine the actual power converted into light. The bulb is rated at 150 watt, which means it consumes 150 Joules of energy per second ($150 \text{ J/s}$). However, only 8% of this energy is converted into light.
Power converted to light ($P_{light}$) is calculated as:
$ P_{light} = P_{total} \times \text{efficiency} $
Where:
Substituting the values:
$ P_{light} = 150 \text{ J/s} \times 0.08 = 12 \text{ J/s} $
So, the bulb emits 12 Joules of light energy every second.
Next, we use the energy of a single photon to find out how many photons make up this light energy emitted each second.
The energy of one photon ($E_{photon}$) is given as $4.42 \times 10^{-19} \text{ J}$.
The number of photons emitted per second ($N$) can be found by dividing the total light power ($P_{light}$) by the energy per photon ($E_{photon}$):
$ N = \frac{P_{light}}{E_{photon}} $
Substitute the known values:
$ N = \frac{12 \text{ J/s}}{4.42 \times 10^{-19} \text{ J/photon}} $
Now, perform the calculation:
$ N = \frac{12}{4.42} \times 10^{19} \text{ photons/s} $
$ N \approx 2.7149 \times 10^{19} \text{ photons/s} $
Rounding to two decimal places, we get approximately $2.71 \times 10^{19}$ photons per second.
Match List I with List II :
List I (Quantum Numbers ) $n$, $l$ | List II (Orbital) |
| A. 2, 1 | I. 3d |
| B. 4, 0 | II. 2p |
| C. 5, 3 | III. 4s |
| D. 3, 2 | IV. 5f |
Choose the correct answer from the options given below :
| List I (Order of reaction) | List II (Unit of rate constant) |
| A. Zero order | I. $mol^{-1} L s^{-1}$ |
| B. First order | II. $mol^{-2} L^2 s^{-1}$ |
| C. Second order | III. $s^{-1}$ |
| D. Third order | IV. $mol L^{-1} s^{-1}$ |
At 298 K, a certain buffer solution contains equal concentrations of $X^{-}$ and $HX$. $K_b$ for $X^-$ is $10^{-10}$. What is the pH of this buffer solution ?
Consider the following reaction :
$2A (g) + B (g) \rightarrow 2D (g)$
$\Delta U^\ominus = -10 \text{ kJ mol}^{-1}$ and $\Delta S^\ominus = -44 \text{ J K}^{-1}$ at 298 K.
Identify the correct option with $\Delta G^\ominus$ for the reaction and spontaneity of the reaction at 298 K. (Given : $R = 8.31 \text{ J mol}^{-1} \text{K}^{-1}$)