Balance each of the following: (please add 1 where needed - even though we usually do not) 1) 1 NaHCO3 (s) ----> 1 2) 1 NaHCO3 (s) ----> 1 1 NaHCO3 (s)----> 1 3) 2 1 4) 2 NaHCO3 (s) ----> 1 H2(g) + 2 C(s) + 3 02(g) Using a mass of 1.70 g baking soda you started with initially, calculate the mass (g) of solid product that should be produced for equation 3 above. Answer with two decimal places and do not include units. Please use: Na = 22.99; H = 1.008; C = 12.011 and O = 15.999 g/mole. 31.02 Using a mass of 0.63 g baking soda you started with initially, calculate the mass (g) of solid product that should be produced for equation 4 above. Answer with two decimal places and do not include units. Please use: Na = 22.99; H = 1.008; C = 12.011 and O = 15.999 g/mole. 0.26 H2O(g) H₂O(g) 2 NaOH (s) + Na2CO3(s) + + 2 Na(s) + Na2O(s) 1 1 CO2(g) CO2(g) CO2(g)
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?
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