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Consider the following reaction
OF2(g) + H2O(g) --- > 2 HF(g) + O2(g) ∆Hºrxn(kJ/mole)= -318 kJ/mole
- Using this information along with data in the appendix of your textbook, calculate
∆Hºf(OF2(g)) in kJ/mole at 25oC.
(b) If 15.0 g of OF2(g) and 10.0 g of H2Og) react, how much heat, expressed in kJ is released?
Hint: First calculate the limiting reagent.
Homework Answers
5. (20 pts) Consider the following reaction OF2(g) + H2O(g) ---> 2 HF(g) + O2(g) AH.(kJ/mole)=-318 kJ/mole (a) U...
5. (20 pts) Consider the following reaction OF2(g) + H2O(g) ---> 2 HF(g) + O2(g) AH.(kJ/mole)=-318 kJ/mole (a) Using this information along with data in the appendix of your textbook, calculate AH (OF,(g)) in kJ/mole at 25°C. (b) If 15.0 g of OF2(g) and 10.0 g of H2Og) react, how much heat, expressed in kJ is released? Hint: First calculate the limiting reagent.
5. (20 pts) Consider the following reaction OF2(g) + H2O(g) ---> 2 HF(g) + O2(g) AH.(kJ/mole) -318 kJ/mole (a) U...
5. (20 pts) Consider the following reaction OF2(g) + H2O(g) ---> 2 HF(g) + O2(g) AH.(kJ/mole) -318 kJ/mole (a) Using this information along with data in the appendix of your textbook, calculate AH;(OF,(8)) in kJ/mole at 25°C. (b) If 15.0 g of OF2(g) and 10.0 g of H2Og) react, how much heat, expressed in kJ is released? Hint: First calculate the limiting reagent. 6.(20 pts) Consider two Styrofoam coffee cups. If cup #1 contains 102.0 mL of water at 81.8°C...
5. (20 pts) Consider the following reaction OF:(g)+ H20(g) (a) Using this information along with data...
5. (20 pts) Consider the following reaction OF:(g)+ H20(g) (a) Using this information along with data in the appendix of your textbook, calculate AH(OF, (g)) in kJ/mole at 25 C. (b) If 15.0 g of OF (g) and 10.0 g of H2Og) react, how much heat, expressed in kJ is released? Hint: First calculate the limiting reagent. 2 HF(g) + O(g) AH (kJ/mole)--318 kJ/mole Consider two Styrofoam coffee cups. If cup # 1 contains 102.0 mL of water at 81.8...
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Calculate ΔHrxno (kJ/mole) for the reaction C2H4(g) + 6 F2(g) ----- > 2 CF4(g) + 4 HF(g) ΔHrxno (kJ/mole) = ? Using only the following data ∆Hºrxn(kJ/mole) H2(g) + F2(g) ------ > 2 HF(g) -537.0 C(s) + 2 F2(g) ----- > CF4(g) - 680.0 2 C(s) + 2 H2(g) ----- > C2H4(g) + 52.3
At what temperature will a 13.7 g Cl2 sample exert a pressure of 0.993 bar when...
At what temperature will a 13.7 g Cl2 sample exert a pressure of 0.993 bar when confined in a 7.50L container? It is found that 6.00 g of potassium metal reacts with excess water to release 29.8 kJ of heat. This means that, for the reaction: 2K(s) + 2H2O(l) à 2KOH(aq) + H2(g) What is the enthalpy of reaction per mole of potassium metal? 2. The overall reaction in a commercial heat pack can be represented as: 4Fe(s) + 3O2(g)...
Information from the appendix is attached: 5. (20 pts) Consider the following reaction OF2(g) + H2O(g)...
Information from the appendix is attached:
5. (20 pts) Consider the following reaction OF2(g) + H2O(g) ---> 2 HF(g) + O2(g) AH (kJ/mole) = -318 kJ/mole (a) Using this information along with data in the appendix of your textbook, calculate AH (OF, (g)) in kJ/mole at 25°C. (b) If 15.0 g of OF2(g) and 10.0 g of H2Og) react, how much heat, expressed in kJ is released? Hint: First calculate the limiting reagent. 6.(20 pts) Consider two Styrofoam coffee cups....
Calculate the in kJ/mole given that the following reaction has a = -1219.26 kJ/mol 2 ClF3(g)...
Calculate the in kJ/mole given that the following reaction has a = -1219.26 kJ/mol 2 ClF3(g) + 2 NH3(g) ----- > N2(g) + 6 HF(g) + Cl2(g) Use data in appendix III (b) The military uses FRH’s (Flameless ration heaters) to heat MRE’s (meals ready to eat). (Heat of formation of Mg( OH)2(Aqua) = -926.8 kJ/mole One of the reactions used in an FRH is Mg(s) + 2 H2O(l) ------ > Mg(OH)2(aq) + H2(g) Using data in Appendix III...
#4.(25pts) Consider the reaction AH (kJ/mole) 5 CO2(g) + SizN() ----> 3 SiO(g) + 2 N2O(s)...
#4.(25pts) Consider the reaction AH (kJ/mole) 5 CO2(g) + SizN() ----> 3 SiO(g) + 2 N2O(s) + 5 CO(g) AH = 2023.75 kJ/mole (1) Use the above information as well as heat of formation data in the appendix of your textbook to calculate AH (Si,N.(s)) in kJ/mole. Additional information: AH (SiO(g)) = 1.94 x 109 kJ/mole 6) How many kJ of heat are absorbed when 1.2 lbs of Si N.(s) react according to the above equation? 1 lb = 453.6...
Given the following thermochemical equation, calculate the amount of heat (in kJ) that is released when...
Given the following thermochemical equation, calculate the amount of heat (in kJ) that is released when 35.0 g of Na2O2 completely react with excess amount of water . 2 Na2O2 (s) + 2 H2O (l) → 4 NaOH (aq) + O2 (g) Δ H = - 126 kJ
5. Yoptional) The Solvay process is used to manufacture baking soda, NaHCO3. In the process, CO2,...
5. Yoptional) The Solvay process is used to manufacture baking soda, NaHCO3. In the process, CO2, NH3, H2O, and NaCl react to produce baking soda. If 15.0 L CO2 and 10.0 NH3 react at STP, with excess water and sodium chloride, what is the limiting reactant? Calculate the mass of baking soda produced. CO2(g) + NH3(g) + H2O(l) + NaCl(s) + NaHCO3(s) + NH4Cl(aq) Mass NaHCO3 Limiting Reactant
5. (20 pts) Consider the following reaction OF2(g) + H2O(g) ---> 2 HF(g) + O2(g) AH.(kJ/mole)=-318 kJ/mole (a) Using this information along with data in the appendix of your textbook, calculate AH (OF,(g)) in kJ/mole at 25°C. (b) If 15.0 g of OF2(g) and 10.0 g of H2Og) react, how much heat, expressed in kJ is released? Hint: First calculate the limiting reagent.
5. (20 pts) Consider the following reaction OF2(g) + H2O(g) ---> 2 HF(g) + O2(g) AH.(kJ/mole) -318 kJ/mole (a) Using this information along with data in the appendix of your textbook, calculate AH;(OF,(8)) in kJ/mole at 25°C. (b) If 15.0 g of OF2(g) and 10.0 g of H2Og) react, how much heat, expressed in kJ is released? Hint: First calculate the limiting reagent. 6.(20 pts) Consider two Styrofoam coffee cups. If cup #1 contains 102.0 mL of water at 81.8°C...
5. (20 pts) Consider the following reaction OF:(g)+ H20(g) (a) Using this information along with data in the appendix of your textbook, calculate AH(OF, (g)) in kJ/mole at 25 C. (b) If 15.0 g of OF (g) and 10.0 g of H2Og) react, how much heat, expressed in kJ is released? Hint: First calculate the limiting reagent. 2 HF(g) + O(g) AH (kJ/mole)--318 kJ/mole Consider two Styrofoam coffee cups. If cup # 1 contains 102.0 mL of water at 81.8...
Information from the appendix is attached:
5. (20 pts) Consider the following reaction OF2(g) + H2O(g) ---> 2 HF(g) + O2(g) AH (kJ/mole) = -318 kJ/mole (a) Using this information along with data in the appendix of your textbook, calculate AH (OF, (g)) in kJ/mole at 25°C. (b) If 15.0 g of OF2(g) and 10.0 g of H2Og) react, how much heat, expressed in kJ is released? Hint: First calculate the limiting reagent. 6.(20 pts) Consider two Styrofoam coffee cups....
#4.(25pts) Consider the reaction AH (kJ/mole) 5 CO2(g) + SizN() ----> 3 SiO(g) + 2 N2O(s) + 5 CO(g) AH = 2023.75 kJ/mole (1) Use the above information as well as heat of formation data in the appendix of your textbook to calculate AH (Si,N.(s)) in kJ/mole. Additional information: AH (SiO(g)) = 1.94 x 109 kJ/mole 6) How many kJ of heat are absorbed when 1.2 lbs of Si N.(s) react according to the above equation? 1 lb = 453.6...
5. Yoptional) The Solvay process is used to manufacture baking soda, NaHCO3. In the process, CO2, NH3, H2O, and NaCl react to produce baking soda. If 15.0 L CO2 and 10.0 NH3 react at STP, with excess water and sodium chloride, what is the limiting reactant? Calculate the mass of baking soda produced. CO2(g) + NH3(g) + H2O(l) + NaCl(s) + NaHCO3(s) + NH4Cl(aq) Mass NaHCO3 Limiting Reactant
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