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k0ka [10]
3 years ago
10

What are the products of photosynthesis?

Chemistry
2 answers:
77julia77 [94]3 years ago
8 0
Carbon dioxide and water pretty sure
aksik [14]3 years ago
8 0
Answer:

Carbon dioxide and water!!!!!!!!!!

Explanation:
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Why is Helium considered a stable element
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3 years ago
Calculate the amount of energy (in kilojoules) needed to heat 346 g of liquid water from –10 °C to 182°C. Assume that the specif
TiliK225 [7]

Answer : The amount of heat required is, 1.16\times 10^6J

Solution :

The process involved in this problem are :

(1):H_2O(s)(-10^oC)\rightarrow H_2O(s)(0^oC)\\\\(2):H_2O(s)(0^oC)\rightarrow H_2O(l)(0^oC)\\\\(3):H_2O(l)(0^oC)\rightarrow H_2O(l)(100^oC)\\\\(4):H_2O(l)(100^oC)\rightarrow H_2O(g)(100^oC)\\\\(5):H_2O(g)(100^oC)\rightarrow H_2O(g)(182^oC)

The expression used will be:

\Delta H=[m\times c_{p,s}\times (T_{final}-T_{initial})]+m\times \Delta H_{fusion}+[m\times c_{p,l}\times (T_{final}-T_{initial})]+m\times \Delta H_{vap}+[m\times c_{p,g}\times (T_{final}-T_{initial})]

where,

\Delta H = heat required for the reaction

m = mass of ice = 346 g

c_{p,s} = specific heat of solid water or ice = 2.09J/g^oC

c_{p,l} = specific heat of liquid water = 4.184J/g^oC

c_{p,g} = specific heat of gaseous water = 1.99J/g^oC

\Delta H_{fusion} = enthalpy change for fusion = 333J/g

\Delta H_{vap} = enthalpy change for vaporization = 2260J/g

Now put all the given values in the above expression, we get:

\Delta H=[346g\times 2.09J/g^oC\times (0-(-80))^oC]+346g\times 333J/g+[346g\times 4.184J/g^oC\times (100-0)^oC]+346g\times 2260J/g+[346g\times 1.99J/g^oC\times (180-100)^oC]

\Delta H=1.16\times 10^6J

Therefore, the amount of heat required is, 1.16\times 10^6J

4 0
3 years ago
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