Carbon dioxide gas and liquid water form solid glucose (C6H12O6) and oxygen gas during photosynthesis. Chlorophyll absorbs light in the 600-700 nm region.

a) Write a balanced thermochemical equation for the formation of 1.00 mol of glucose.
... I know that it goes like this: 6CO2(g)+6H2O(l)-->C6H12O6(s)+6O2(g)... this is already balanced but not yet considered a "thermochemical equation"

b) What is the minimum number of photons with Y=680 nm needed to form 1.00 mol of glucose?

I think the delta Ho formation for glucose is about 3000 kJ/mol glucose but you need to look it up. I don't have all of these dH values memorized. Then

6CO2 + 6H2O + light energy --> C6H12O6 + 6O2 delta H = +3000 kJ/mol

For wavelength = 680 nm, convert to E with
E = h*c/wavelength which gives you J/photon. and convert that to photons needed for approx 3000 kJ/mol glucose.

To answer this question, we need to consider the molar ratio between the reactants and products in the thermochemical equation for photosynthesis. From the equation, we can see that 6 moles of carbon dioxide (CO2) are required to form 1 mole of glucose (C6H12O6).

a) Based on this information, we can write the balanced thermochemical equation for the formation of 1.00 mol of glucose as follows:

6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g)

Note that the equation is already balanced.

b) To determine the minimum number of photons with a wavelength of 680 nm needed to form 1.00 mol of glucose, we need to consider the concept of photon energy and the relationship between energy and wavelength.

The energy of a photon can be calculated using the equation:

E = (hc)/λ

where E represents energy, h is Planck's constant (6.62607015 × 10-34 joule-seconds), c is the speed of light (3.00 × 10^8 meters/second), and λ is the wavelength in meters.

To convert 680 nm to meters, we divide the wavelength by 10^9:

λ = 680 nm / (10^9 m/nm)

Now we can calculate the energy of a single 680 nm photon using the equation:

E = (6.62607015 × 10-34 J·s) × (3.00 × 10^8 m/s) / (680 × 10^-9 m)

This gives us the energy per photon. To find the minimum number of photons needed to form 1.00 mol of glucose, we calculate the total energy required for glucose formation and divide it by the energy per photon:

Total Energy = Energy per photon × Number of photons

Total Energy = (Energy per photon) × (Number of photons)

Number of photons = Total Energy / Energy per photon

The total energy required for the reaction can be calculated from the enthalpy change of the reaction, which is usually given in thermochemical equations. In this case, however, we don't have the enthalpy change and need to make some assumptions.

Let's assume that the reaction is exothermic, meaning it releases energy. In this case, we can assume that the energy required for the reaction is equivalent to the energy released when 1.00 mol of glucose is formed. We can then use the standard enthalpy of formation of glucose (ΔHƒ) to calculate the total energy required.

Assuming ΔHƒ for glucose is -2802.3 kJ/mol, we can convert it to joules:

ΔHƒ = -2802.3 kJ/mol × (1000 J/1 kJ) = -2802300 J/mol

Now we can calculate the number of photons required:

Number of photons = (-2802300 J/mol) / (Energy per photon)

Plugging in the value for the energy per photon calculated earlier, we can find the minimum number of photons required to form 1.00 mol of glucose.

Please note that this calculation assumes ideal conditions and may not accurately represent the complex process of photosynthesis in real-life scenarios.

To determine the minimum number of photons with a wavelength of 680 nm that are needed to form 1.00 mol of glucose, we need to calculate the energy required for this reaction.

First, we can calculate the energy of a single photon using the equation:

E = hc/λ

Where:
E = Energy of a photon
h = Planck's constant (6.626 x 10^-34 J·s)
c = Speed of light (3.00 x 10^8 m/s)
λ = Wavelength of the photon (680 nm = 6.80 x 10^-7 m)

Now, we can calculate the energy required to produce 1.00 mole of glucose. Since the balanced equation tells us that 6 moles of carbon dioxide reacts to form 1 mole of glucose, we will multiply the energy of one photon by 6:

Energy required = 6 * (hc/λ)

Plugging in the values:

Energy required = 6 * ((6.626 x 10^-34 J·s) * (3.00 x 10^8 m/s) / (6.80 x 10^-7 m))

Now, we can calculate the energy required using the equation:

Energy required ≈ 1.92 x 10^-19 J

Therefore, the minimum number of photons with a wavelength of 680 nm needed to form 1.00 mole of glucose is approximately 1.92 x 10^-19 photons.