Predict the products of the reaction below. That is, complete the right-hand side of the chemical equation. Be sure your equation is balanced. HC10, + NaOH ||
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- When ethanol (CH3CH2OH) burns in oxygen, carbon dioxide and water are formed. (i) Write the equation which describes this reaction. (ii) Using the data below, calculate the value for ∆Ho for the combustion of ethanol. Hof (CH3CH2OH(l)) = - 277.0 kJmol-1 Hof (CO2(g)) = - 393.7 kJmol-1Hof (H2O(l)) = - 285.9 kJmol-1Chemistry Inside a body, this reaction has a value of positive ∆G C6H12O6 + H3PO4 → C6H14O12P2 + H2O ∆G= +13.4 kJ/mol Can you show me how to keep this reaction going in living things? Prove it with calculations.Carbon dioxide from the atmosphere “weathers”, or dissolves, limestone, CaCO3 by thereaction.CaCO3 (s) + CO2 (g) + H2O (l) → Ca2+ (aq) + 2 HCO3- (aq)What is DH° for this reaction? DH°f CaCO3 (s) = -1206.9 kJ/mol, DH°f CO2 (g) = -393.5 kJ/mol,DH°f H2O (l) = -285.8 kJ/mol, DH°f Ca2+ (aq) = -542.8 kJ/mol, DH°f HCO3 (aq) = -692.0 kJ/mol
- The heating of CuSO4. 5H2O(S) yields several transitions as a function of temperature. The table below gives the percentage of original mass lost as a function of the approximate temperature. Use these percentages to determine the sequence of decompositions and write chemical equations for each transition. percentage of original mass lost 14.5 29.0 36.0 51.5 67.0 70.5 approximate temperature (Degree C) 100 130 220 800 910 1020Prof. Neiman and Prof. James were first to discovered in 1973 that chlorofluorocarbons (CFCs) were depleting the Earth’sozone layer when released into the atmosphere. Once they reach the stratosphere, Clis released from the CFCs molecules by interaction with UV light. Free Cl atoms areable to react with ozone in a catalytic cycle that converts O3into the more stable O2.It is estimated that a single Cl atom is able to react with∼100000 O3molecules.Although CFCs production was banned in 1996, there are still a substantial numberof motor vehicle air conditioners (MVACs) that use CFC-12 (CF2Cl2) as refrigerant.The average CFC-12 emission rate from operating MVACs has been estimated tobe 59.5 mg per hour per vehicle (Zhang et al.Environ. Sci. Technol. Lett.2017).How much chlorine, in kg, is added to the atmosphere in a year due to 100 millionMVACs using CFC-12 as refrigerant?Hw.34. show how to balance equation...
- For the arrhenius equation what are the derivations to solve for T1, T2, K1, K2, Ea since its easier for me to just plug in the numbers in that manner since im not good at math. It doesnt have to be the one I have added below its just an example.I need help balancing equation(e) on the file attached belowUCI Chemistry researchers, Prof. F. Sherwood Rowland and Dr. Mario Molina werefirst to discovered in 1973 that chlorofluorocarbons (CFCs) were depleting the Earth’sozone layer when released into the atmosphere. Once they reach the stratosphere, Clis released from the CFCs molecules by interaction with UV light. Free Cl atoms areable to react with ozone in a catalytic cycle that converts O3into the more stable O2.It is estimated that a single Cl atom is able to react with∼100000 O3molecules.Although CFCs production was banned in 1996, there are still a substantial numberof motor vehicle air conditioners (MVACs) that use CFC-12 (CF2Cl2) as refrigerant.The average CFC-12 emission rate from operating MVACs has been estimated tobe 59.5 mg per hour per vehicle (Zhang et al.Environ. Sci. Technol. Lett.2017).How much chlorine, in kg, is added to the atmosphere in a year due to 100 millionMVACs using CFC-12 as refrigerant?
- Determine rxnH 25 C for the following reaction: NO g O2 g NO2 g This reaction is a major participant in the formation of smog.Consider the following reactions at 25◦C:reaction Kc2 NO(g) ⇀↽ N2(g) + O2(g) 1 × 10302 H2O(g) ⇀↽ 2 H2(g) + O2(g) 5 × 10−822 CO(g) + O2(g) ⇀↽ 2 CO2(g) 3 × 1091Which compound is most likely to dissociateand give O2(g) at 25◦C?1. CO2. CO23. NO4. H2OREPOST please help with reaction 2 and 3 under calculations (for reaction 2 help had been provide till part 3 Note: Since you have posted a question with multiple sub-parts, we will provide the solution only to the first three sub-parts as per our Q&A guidelines. Please repost the remaining sub-parts separately. Given that: Initial temperature, T1 = 24.0oC Final temperature, T2 = 32.1oC Volume of HCl = 100 mL Density of HCl = 1 g/mL Concentration of HCl = 1.0 mol/L = 1.0 M arrow_forward Step 2 1.) The change in temperature is calculated using the following expression: ∆T=Final temprature-Initial temperature=T2-T1 Substitute 32.1oC for T2, and 24.0oC for T1 in the above expression to calculate the change in temperature for reaction 2. ∆T=32.1°C-24.0°C=8.1°C arrow_forward Step 3 2.) The formula to calculate the mass of a substance is written as follows: Mass=Volume×Density Substitute 100 mL for the volume and 1 g/mL for the density in the above formula to calculate the…