Sodium carbonate is used to manufacture glass. It is obtained by heating sodium bicarbonate as follows:...
Sodium carbonate is used to manufacture glass. It is obtained by heating sodium bicarbonate as follows: 2 NaHCO3 (s) → Na2CO3 (s) + H2O (g) + CO2 (g) ΔH = +129.3 kJ This reaction is (endothermic/exothermic). How many grams of sodium carbonate are produced if 1252 kJ of heat are used to decompose the sodium bicarbonate? g Na2CO3 (4 SF) How much heat is required to decompose 15.65 grams of NaHCO3? kJ (4 SF) Blank 1: Blank 2: Blank 3:
Homework Answers
2 NaHCO3 (s) → Na2CO3 (s) + H2O (g) + CO2 (g) ΔH = +129.3 kJ
The amount of energy is required for decomposition of NaHCO3 . So in this reaction heat energy is absorbed. It is endothermic reaction . For endothermic reaction ΔH is positive .
This reaction is endothermic >>>>answer
129.3KJ energy is used for formation of 1 mole of Na2CO3
129.3KJ energy is used for formation of 106g of Na2CO3
1252Kj energy is used for formation of = 106*1252/129.3 = 1026.38g of Na2CO3 >>>>>answer
2 moles of NaHCO3 decomposes to absorbed heat energy is 129.3KJ
2*84g of NaHCO3 decomposes to absorbed heat energy is 129.3Kj
15.65g of NaHCO3 decomposes to absorbed heat energy = 129.3*15.65/(2*84) = 12.045g of NaHCO3 >>>>answer
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Sodium carbonate is used to manufacture glass. It is obtained by
heating sodium bicarbonate as follows:...
Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g)...
Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g) Given that ΔH° = 128.9 kJ and ΔG° = 33.1 kJ at25°C, above what minimum temperature will the reaction becomespontaneous under standard state conditions?
Upon heating, sodium bicarbonate decomposes into sodium carbonate, carbon dioxide, and water vapor according to the...
Upon heating, sodium bicarbonate decomposes into sodium carbonate, carbon dioxide, and water vapor according to the following chemical reaction: 2 NaHCO3 (s) →→ Na2CO3 (s) + CO2 (g) + H2O (g) If the initial mass of sodium bicarbonate is 4.859 g, how much sodium carbonate should be produced? a. 3.066 g b. 2.211 g c. 6.131 g d. 4.859 g
At high temperatures, sodium bicarbonate is converted quantitatively to sodium carbonate, producing water and carbon dioxide....
At high temperatures, sodium bicarbonate is converted quantitatively to sodium carbonate, producing water and carbon dioxide. Heating a 1.7184 g sample of impure NaHCO3 produces 0.196 grams of CO2. Determine the mass percent of sodium bicarbonate in the original mixture. (Assume the impurities do not decompose when heated.)
Solid sodium hydrogen carbonate, NaHCO3, decomposes on heating according to the equation: 2 NaHCO3(s) <-->...
Solid sodium hydrogen carbonate, NaHCO3, decomposes on heating according to the equation: 2 NaHCO3(s) <--> Na2CO3(s) + H2O(g) + CO2(g) A sample of 1.00 x 102 grams of solid NaHCO3 was placed in a previously evacuated rigid 5.00-liter container and heated to 160 0C. Some of the original solid remained and the total pressure in the container was 7.76 atmospheres when equilibrium was reached. Calculate the number of moles of H2O(g) present at equilibrium. How many grams of the...
Write the thermochemical equation that would be used to represent the standard heat of formation of sodium bicarbon...
Write the thermochemical equation that would be used to represent the standard heat of formation of sodium bicarbonate, NaHCO3(s). Na(s) + H2(g) + C(s) + H20(1) NaHCO3(s) AH° = -947.7 kJ/mol Na2O(s) + H2O(g) + CO2(g) + O2(g) + NaHCO3(s) AH = -947.7 kJ/mol O Na(s) + 0.5H2(g) + C(s) + 1.502(g) + NaHCO3(s) AH = -947.7 kJ/mol Na2CO3(s) + H20(1) - NaHCO3(s) AH = -947.7 kJ/mol
1.Sodium hydrogen carbonate, NaHCO3, can be decomposed completely by heating. 2 NaHCO3(s) → Na2CO3(s) + CO2(g)...
1.Sodium hydrogen carbonate, NaHCO3, can be decomposed completely by heating. 2 NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g) A sample of impure NaHCO3 with an initial mass of 0.739 g yielded a solid residue (consisting of Na2CO3 and other solids) with a final mass of 0.564 g. Determine the mass percent of NaHCO3 in the sample. 2.In a process for producing acetic acid, oxygen gas is bubbled into acetaldehyde, CH3CHO, containing manganese(II) acetate (catalyst) under pressure at 60°C. 2CH3CHO(l) +...
Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to...
Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HC1), which the stomach secretes to help digest food. Drinking a glass of water containing dissolve NaHCO3 neutralizes excess HCl through this reaction: HCI(aq) NaHCO3(aq) → NaCl(aq) + H,O() + CO2(g) The CO2 gas produced is what makes you burp after drinking the...
Single Replacement Question 18 1 pts **Show your work on scratch paper A student performed the...
Single Replacement Question 18 1 pts **Show your work on scratch paper A student performed the stoichiometry lab' and investigated the decomposition of sodium bicarbonate by heating a sample of sodium bicarbonate in a crucible. They began the lab with a 4.234 gram sample of sodium bicarbonate. If the student assumed that the below! reaction that took place (producing sodium carbonate), what would be the theoretical yield of sodium carbonate? 2 NaHCO3(s) Na2CO3(s) + CO2(g) + H2O (8) 5.342 grams...
sodium carbonate can be made by heating sodiumbicarbonate: 2NaHCO3(s) --> Na2CO3(s) +CO2(g) + H2O(g) Given that...
sodium carbonate can be made by heating sodiumbicarbonate: 2NaHCO3(s) --> Na2CO3(s) +CO2(g) + H2O(g) Given that ΔHo = 128.9 kJ/mol andΔGo = 33.1 kJ/mol at 25oC, above whatminimum temperature will the reaction become spontaneous understandard state conditions? I know the answer is 401 K but I don't know how to get theanswer. If you could please show me step by step I will ratelifesaver.
PART ONE: Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be...
PART ONE: Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in...
Write the thermochemical equation that would be used to represent the standard heat of formation of sodium bicarbonate, NaHCO3(s). Na(s) + H2(g) + C(s) + H20(1) NaHCO3(s) AH° = -947.7 kJ/mol Na2O(s) + H2O(g) + CO2(g) + O2(g) + NaHCO3(s) AH = -947.7 kJ/mol O Na(s) + 0.5H2(g) + C(s) + 1.502(g) + NaHCO3(s) AH = -947.7 kJ/mol Na2CO3(s) + H20(1) - NaHCO3(s) AH = -947.7 kJ/mol
Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HC1), which the stomach secretes to help digest food. Drinking a glass of water containing dissolve NaHCO3 neutralizes excess HCl through this reaction: HCI(aq) NaHCO3(aq) → NaCl(aq) + H,O() + CO2(g) The CO2 gas produced is what makes you burp after drinking the...
Single Replacement Question 18 1 pts **Show your work on scratch paper A student performed the stoichiometry lab' and investigated the decomposition of sodium bicarbonate by heating a sample of sodium bicarbonate in a crucible. They began the lab with a 4.234 gram sample of sodium bicarbonate. If the student assumed that the below! reaction that took place (producing sodium carbonate), what would be the theoretical yield of sodium carbonate? 2 NaHCO3(s) Na2CO3(s) + CO2(g) + H2O (8) 5.342 grams...
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