Answer:
The right answer is "8.81 atm".
Explanation:
Given:
V = 5.00 L
Mass = 4900 g
MW = 32 g/mol
T = 350 K
Now,
Number of moles will be:
By using the ideal gas equation, we get
⇒
or,
⇒
By substituting the values, we get
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Answer:
The total photons required = 5.19 × 10²⁸ photons
Explanation:
Given that:
the radiation wavelength λ= 12.5 cm = 0.125 m
Volume of the container = 0.250 L = 250 mL
The density of water = 1 g/mL
Density = mass /volume
Mass = Volume × Density
Thus; the mass of the water = 250 mL × 1 g/mL
the mass of the water = 250 g
the specific heat of water s = 4.18 J/g° C
the initial temperature = 20.0° C
the final temperature = 99° C
Change in temperature = (99-20)° C = 79 ° C
The heat q absorbed during the process = ms
The heat q absorbed during the process = 250 g × 4.18 J/g° C × 79° C
The heat q absorbed during the process = 82555 J
The energy of a photon can be represented by the equation :
= hc/λ
where;
h = planck's constant =
c = velocity of light =
=
= J
The total photons required = Total heat energy/ Energy of a photon
The total photons required =
The total photons required = 5.19 × 10²⁸ photons
Answer: m = 11.2 g C7H16
Explanation: First convert the mass of CO2 to moles. Then do the mole ratio between CO2 and C7H16 which is 7:1. Finally convert the moles of C7H16 to the mass of C7H16.
Solution attached.
