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1 answer:
(a) 33.6 L of oxygen would be produced.
(b) 106 grams of would be needed
1 mole of gas = 22.4 L
(a) From the equation, 2 moles of produce 3 moles of
. 1 mole of
will, therefore, produce 1.5 moles of
.
1.5 moles of oxygen = 22.4 x 1.5 = 33.6 L
(b) 22.4 L of is produced at STP. This means that 1 mole of the gas is produced.
From the equation, 1 mole of requires 1 mole of
.
Molar mass of = (23x2)+ (12)+(16x3) = 106 g/mol
Mass of 1 mole = 1 x 106 = 106 grams
More on stoichiometric calculations can be found here: brainly.com/question/27287858
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The given question is incomplete. The complete question is :
It takes 151 kJ/mol to break an iodine-iodine single bond. Calculate the maximum wavelength of light for which an iodine-iodine single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.
Answer: 793 nm
Explanation:
The relation between energy and wavelength of light is given by Planck's equation, which is:
where,
E = energy of the light = 151 kJ= 151000 J (1kJ=1000J)
N= moles = 1 =
h = Planck's constant =
c = speed of light =
= wavelength of light = ?
Putting in the values:
Thus the maximum wavelength of light for which an iodine-iodine single bond could be broken by absorbing a single photon is 793 nm