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- Carbon monoxide poisoning results when carbon monoxide replaces oxygen bound to hemoglobin. The oxygenated form of hemoglobin, HbO2 carries O2 to the lungs. HbO2(aq)+CO(g)HbCO(aq)+O2(g) At 98.6°F (37°C), G° for the reaction is about -14 kJ. What is the ratio of [HbO2] to [HbCO] when the pressure of CO is the same as that of O2?During photosynthesis, plants convert carbon dioxide and water to glucose (C6H12O6) and oxygen gas. a. Is photosynthesis a source or a sink of a GHG? Explain. b. Write and balance the chemical equation for the photosynthesis c. It is estimated that the amount of CO2 sequestered (removed from the air) by an urban tree is 60.0 kg.4 How much glucose can be produced from 60.0 kg CO2 during photosynthesis?Suppose that H2O (l) goes from 29.0oC and 1 atm to 31.0oC and pressure P2. What value of P2 would make ∆S=0 for this process?
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- Consider the reaction between methane and oxygen producing carbon dioxide and water. Suppose that the reaction is carried out in a furnace used to heat a house. If q=890kJ and w=+5kJ, what is E? H at 25C?is the following statement correct?Trinitroglycerin, C3H5N3O9C3H5N3O9 (usually referred to simply as nitroglycerin), has been widely used as an explosive. Alfred Nobel used it to make dynamite in 1866. Rather surprisingly, it also is used as a medication, to relieve angina (chest pains resulting from partially blocked arteries to the heart) by dilating the blood vessels. At 1 atm pressure and 25°C, the enthalpy of decomposition of trinitroglycerin to form nitrogen gas, carbon dioxide gas, liquid water, and oxygen gas is -1541.4 kJ/mol. (a) Write a balanced chemical equation for the decomposition of trinitroglycerin. (b) Calculate the standard heat of formation of trinitroglycerin. (c) A standard dose of trinitroglycerin for relief of angina is 0.65 mg. If the sample is eventually oxidized in the body to nitrogen gas, carbon dioxide gas, and liquid water, how many joules of energy is released? (d) If 2.5 calories is released upon the oxidation of trinitroglycerin in the body, how many μg of trinitroglycerin was…
- Trinitroglycerin, C3H5N3O9C3H5N3O9 (usually referred to simply as nitroglycerin), has been widely used as an explosive. Alfred Nobel used it to make dynamite in 1866. Rather surprisingly, it also is used as a medication, to relieve angina (chest pains resulting from partially blocked arteries to the heart) by dilating the blood vessels. At 1 atm pressure and 25°C, the enthalpy of decomposition of trinitroglycerin to form nitrogen gas, carbon dioxide gas, liquid water, and oxygen gas is -1541.4 kJ/mol. Calculate the standard heat of formation of trinitroglycerin. (step by step)During the industrial synthesis of methanol (CH3OH), carbon monoxide (CO) reactswith hydrogen gas. For methanol, ΔH= -100.4 kJ/mol. a. Write the balanced chemical equation for this reaction.b. Is it better to maintain this system at a low or high temperature, to obtain agood output? Explain.What is the total heat of reaction of the decomposition of C3H8 at 693.15 K. The reaction is 0.69 conversion of C3H8. Express answer in kJ per mol C3H8 decomposed.