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4 KO2(s) + 2 CO2(g) -------> 2 K2CO3(s) + 3 O2(g) How many grams of KO2 are needed to produce 824.0 L of O2 at 13.0 °C and 1.00 atm?
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp for the reaction at 298 K. A. 7.63 x 10-7 B 660 C. 54 D. 2.74 x 104 10 E Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp...
Using the equations below: C(s) + O2(g) → CO2(g) AH = -390 KJ Mn(s) + O2(g) → MnO2(s) AH = -520 KJ What is the AH (in K)) for the following reaction? MnO2(s) + C(s) + Mn(s) + CO2(g) : AH = ? Hint: Use Hess's law O A. 910 KJ B. -130 KJ C. 130 KJ OD. -910 KJ
1) Find the AH of the following reaction: C(s) + O2(g) à CO2(g) Given the following data: Sro(s) + CO2(g) à SrCO3(s) 2Sro(s) à 2Sr(s) +0,(8) AH = -234 kJ AH = +1184 kJ 2SCO,(s) à 25r(s) + 2C(s) + 302(g) AH = +2440 kJ 2) Find the AH of the following reaction: 3NO,(g) + H2O(l) à 2HNO,(aq) + NO(g) Given the following data: 2NO(g) + O2(g) à 2NO(g) AH=-116 kJ 2N2(g) + 502(g) + 2H2O(l) à 4HNO3(aq) AH =...
AH = -727 kJ Given that CH3OH (1) + 3/2 O2 (g) → CO2 (g) + 2 H2O(1) CO(g) + 1/2O2 (g) → CO2 (9) CH3OH(1) → CH3OH(g) AH = -284 kJ AH = 38 kJ H20 (1)→ H20 (9) AH = 44 kJ what is AH, in kJ, for the reaction CH3OH (g) + O2(g) →CO (g) + 2 H2O (9)
1) 2) 3) C3H8(g) + 5 O2(g) = 3 CO2(g) + 4H2O(1) AH = -2220 kJ Decreasing the temperature will result in shift the equilibrium to the right shift the equilibrium to the left Keq is decreased O no effect in shifting the equilibrium more information is needed Which of the following expressions is the correct equilibrium-constant expression for the reaction below? P4010(s) = P4(s) + 5 O2(g) [02]-5 O [0215 [P4010] [Pd][02] [P][0215 O [P4010] [P4010) [P][0,1175 A proposed...
Given the following equations and AH' values: C(s) + O2(g) + CO2(g) AH = -393.5 kJ H2(g) + 1/2O2(g) - H20 (1) AH = -285.8 kJ 2C2H2 (8) + 5O2(g) + 4CO2(g) + 2H20 (1) AH'= -2598 kJ Determine the heat of reaction (in kJ) at 298 K for the reaction: 2C(s) + H2(8) C2H2 (8) 0-136.8 0-219.8 0-109.9 O-167.1 +226.2
Potassium superoxide (KO2) reacts with carbon dioxide to produce oxygen in reaction is very fast and nearly quantitative. It is used in submarines, space vehicles, space suits, and by firefighters and miners. 4 KO2(s) + 2 CO2(g) - 2 K2CO3(s) + 3 O2(g) Calculate the mass of KO2 reacted if 355.8 mL of gas is collected over water at 65.0 °C and a barometric pressure of 744.8 torr. (12 pts.) 7. When 12.424 g of (NH4),PO. (FW 149.087 g/mole) is...
Calculate AH for the following reaction, CaO(s) + CO2(g) CaCO3(s) given the thermochemical equations below. 2 Ca(s) + O2(g) + 2 Cao(s) AH = -1270.2 kJ C(s) + O2(g) CO2(g) AH = -393.5 kJ 2 Ca(s) + 2 C(s) + 3 O2(g) → 2 CaCO3(s) AH = -2413.8 kJ 0-750.1 kJ O +350.2 kJ 0 -178.3 kJ O +2870.6 kJ
5. Using standard heats of formation, calculate AH for 4 FeO (s) + O2(g) → 2 Fe2O3 (s) AH1 of FeO (s) = -272.0 kJ/mol AHºf of Fe2O3 (s) = -825.5 kJ/mol 3. Given 3 C (s) + 4 H2(g) → C3H8 (9) AH = -103.85 kJ/mol C(s) + O2(g) + CO2(g) AH = -393.5 kJ/mol H2 (g) + 12 O2(g) → H2O (1) AH = -285.8 kJ/mol find AH for C3H8 (g) + 5 O2(g) → 3 CO2 (g)...