This is a incomplete question. The complete question is:
It takes 348 kJ/mol to break a carbon-carbon single bond. Calculate the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon. Round your answer to correct number of significant digits
Answer: 344 nm
Explanation:
E= energy = 348kJ= 348000 J (1kJ=1000J)
N = avogadro's number = 
h = Planck's constant = 
c = speed of light = 

Thus the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon is 344 nm
<em><u>Answer and Explanation:</u></em>




<em><u>For % of N2 gas:
</u></em>
<em><u /></em>
<em><u /></em>
<em><u /></em>
<em><u /></em>
<em><u /></em>
<em><u /></em>
<em><u /></em>
<em><u /></em>
<em><u /></em>
Answer:
Explanation:
An electron in 4s is farther away from nucleus and it has higher energy when compared to electron from 1s.
Answer: ABC&AMN are congruent by ASA comgruence
angle A=A
sideAN=AB
angle M=C
Explanation:
Answer: 6.1 g
Explanation:
between Mg and MgO theres a 1;1 MOLE RATIO
here's the balanced equation
2Mg + O2 ==> 2MgO
24g of magnesium is approximately 1 mole of magnesium so it produces 40 g of mgo which is also 1 mole of mgo thus 10/40 =0.25 moles of MgO so 0.25 moles of magnesium would be needed which is approximately 6.1 g