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15.47 Which of the following are
a.
b.
c.
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Basic Chemistry
- 18.2 Balance the following chemical equation for the stoichiometric combustion of methane with oxygen. ____ CH4(g) + ______O2(g) ⟶ ______ CO2(g)+ ______H2O(g) What are the coefficients for O2(g) and CO2 (g)?arrow_forward14.60 When iodine is oxidized in concentrated HNO3, it produces the white solid iodic acid, HIO3: L(s)+NO;(aq) HIO3(s)+NO2(g) Balance this equation, adding H*(aq) and H2O(1) as necessary.arrow_forwardFO 2 3) Given the reaction: AB (g) + 2 CD (g) → 3 EF (g) AH = -9.52 kJ How many moles of EF would also be produced if the reaction gave off 750 J? 4) A student mixes 0.100 L of 1.00 M HA with 0.200 L of 1.00 M MOH according to the reaction below: HA (aq) + MOH (aq) → H₂O + MA(aq) a) If the temperature of the solutions changed from 22.3 °C to 29.1 °C, calculate the heat evolved in this reaction. (Assume that the specific heat of the solution is 4.184 J/g°C and the density of the solutions is 1.00 g/mL)arrow_forward
- Part I. Complete the following chemical reactions. Do not forget to balance the reaction, the states of matter and answer any questions that are asked. In the next reaction, a gas is formed. (19 points). HCl (aq) + Mg (s) → Gas that was released: Mg (s) + O2 (g) → Cu2S (s) + O2 (g) → Gas that was released:arrow_forwardWrite the net ionic equation for the reaction of hydrochloric acid with potassium sulfide. 2H+1(aq) + 2S-2(aq) ⟶H2S(g) H+1(aq) + S-2(aq) ⟶H2S(g) H+1(aq) + S-2(aq) ⟶HS(g) 2H+1(aq) + S-2(aq) ⟶H2S(g) 2H+1(aq) + S-2(aq)⟶ H2S(aq)arrow_forward18. Answer the following questions using the given equation and AH. (d) Adding so 6 CO2(g) + 6 H20 (1) → C,H1206(aq) + 6 02(g) AH = +678 kcal/mol (a) Is heat absorbed or released? Chept (b) Are the reactants or products lower in energy? Mult Cho ach) 21. (c) Is the reaction exothermic or endothermic? volume and temperetur somple of ga (d) Which bonds are stronger, those in the reactants or those in the products? (c) Gay-Larrow_forward
- Given the following equation, H₂O(g) + CO(g) → H₂(g) + CO₂(g) What is the AG for the following reaction: 0 +5.72 kJ O+143.0 kJ O-5.72 kJ 5H₂O(g) + 5CO(g) → 5H₂(g) + 5CO2(g) 143.0 kJ O-28.6 kJ AG = -28.6 kJ AG° = ?arrow_forward1.1. For the reaction below, what would cause an increase in NaOH? Maybe more than one correct answer! Mg(OH)2(aq) + 2 Na(s) a) Increase the temperature b) Decrease the temperature g) Decrease Mg(OH)2(aq) 2 NaOH(aq) + Mg(s) c) Increase Na(s) d) Decrease Na(s) AH = -14 kJ/mol e) Adding a catalyst f) Increase Mg(OH)2(aq)arrow_forwardmol/i. 22. Given the reaction: N2 (g) + O2 (g) 2NO (g) Ke = 10.1 at 2000°C If the reaction starts with 0.065 MN2 and 0.065 MO2, what is the equilibrium concentration (M) of NO? (5)arrow_forward
- At high temperatures nitrogen (N2) and oxygen (O2) will react to form NO.N2(g) + O2(g) ⇆ 2 NO(g) (4.1)The value for the equilibrium constant for reaction 4.1 is KC = 2.7 x 10^-17 at some temperature T.A system initially has [N2] = 0.0800 M and [O2] = 0.0500 M. There is no NO initially present inthe system. Find the value for [NO] that will be present at equilibrium.arrow_forwardGive examples of exothermic and endothermic reactions. (5 each)arrow_forwardGiven the following equilibrium constants at 433°C, 1 Na20(s) = 2 Na(1) +02 (9) K1 = 5 x 10-25 2 1 NaO(g) - Na(1)+;02(9) K2 8 x 10-5 -29 Na2 O2 (s) = 2 Na(1) + O2 (9) NaO2 (s) = Na(1) + O2 (9) K3 = 4 × 10 -14 KĄ 3 x 10 determine the values for the equilibrium constants for the following reactions: a. Na20(s) + 1 O2 (g) = Na2 O2 (8) Equilibrium constant = b. NaO(g) + Na, 0(s) = Na2O2(s) + Na(1) Equilibrium constant c. 2 NaO(g) = Na2 O2 (s) Equilibrium constant = (Hint: When reaction equations are added, the equilibrium expressions are multiplied.)arrow_forward
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