The maximum wavelength of light required to break the amide bond is 268 nm. First, we find the average bond energy, then use Avogadro's number to figure out the energy needed for one molecule. Finally, applying the relationship between energy and wavelength, we can conclude the value of the wavelength.
Answer:
0.20M of nitric acid
0.00250M of KSCN
Explanation:
In the case of nitric acid, the solution's dilution changes from 10.00mL to 100.00mL, resulting in a 1/10 dilution. Given the original concentration of nitric acid is 2.0M, the updated concentration becomes: 2.0M×(1/10)=0.20M of nitric acid
Similarly, the dilution of KSCN extends from 50.00mL to 100.00mL, equal to a 1/2 dilution. Consequently, the new concentration of KSCN turns out to be:
0.00500M × (1/2) = 0.00250M of KSCN
I hope it aids you!
1. Stars originate within clouds of gas and dust referred to as nebulas. 2. These clouds are drawn together by gravitational forces. 3. Once sufficient heat and pressure accumulate, nuclear fusion commences, representing the birth of a star.
To determine the mass of salt using Avogadro's number, we find the moles of NaCl: 8.24x10²² molecules NaCl divided by 6.022x10²³ molecules NaCl per mole gives 0.14 mole NaCl. We can convert moles to grams of NaCl by multiplying 0.14 mole by 58g NaCl per mole, yielding a total of 8.12 g NaCl.
Answer:
The temperature increase of the calorimeter, which is missing in the problem, is necessary for the calculation.
Explanation:
Since the temperature rise (X) is unspecified, we'll express the calculation in terms of X, and demonstrate with an example value.
1) Calorimeter details:
- Temperature increase: X °C
- Heat capacity ratio: 4.87 J / 5.5 °C (given)
- Energy absorbed by calorimeter at X °C rise:
(4.87 J / 5.5 °C) × X
2) Reaction data:
- Heat released: 362 kJ per mole of reactant
- Number of moles consumed: n
- Total energy from reaction:
362 kJ/mol × 1000 J/kJ × n = 362,000 n J
3) Using energy conservation, assuming no heat loss to surroundings, the energy from the reaction equals the energy absorbed by the calorimeter:
- 362,000 n = (4.87 J / 5.5 °C) × X
- n = [(4.87 / 5.5) × X] / 362,000
n = 0.000002446 × X
This means for each degree Celsius rise in calorimeter temperature, 0.000002446 moles of reactant were consumed.
Example:
If the calorimeter temperature increases by 100 °C, then:
- n = 0.000002446 × 100 = 0.0002446 mol
