Answer:
1.02KPa
Explanation:
The following were obtained from the question:
V1 = 1550mL
P1 = 70.26kPa
T1 = 480°C = 480 + 273 = 753K
T2 = -237°C = - 237 + 273 = 36K
V2 = 5114mL
P2 =?
The final pressure can obtain as follows:
P1V1/T1 = P2V2/T2
(70.26x1550)/753 = (P2x5114)/36
Cross multiply to express in linear form as shown below:
P2 x 5114 x 753 = 70.26 x 1550 x 36
Divide both side by 5114 x 753
P2 = (70.26x1550x36)/(5114x753)
P2 = 1.02KPa
Therefore, the final pressure is 1.02KPa
That's kind of a ponderous way to describe it, but your 'X' represents
the absolute temperature of the ideal gas.
To calculate this,
We know that energy is 1 photon
E = hc/wavelenth
wavelength of 10.0 m
Solution:
h = 6.626 x 10^-34 Jsec
C = 2.9979 x 10^8 m/sec
E = 6.626 10^-34 * 2.9979 10^8 / 10 = 1.9864 10^-26J
Then, the number of photons is computed by:
n = 1000 / 1.9864 10^-26 = 5.04 10^28 photons
