Hydrogen bromide, HBr, is a colourless gas. Consider its dissociation reaction 2HBr (g) « H2 (g)...

Hydrogen bromide, HBr, is a colourless gas. Consider its dissociation reaction 2HBr (g) « H2 (g) + Br2 (g) DfHo (kJ/mol) -36.4 +30.9 So (J/K.mol) +198.7 +130.7 +245.5 ooo a) Determine DeltaH , DeltaS , DeltaG , and Kp (all at T= 298 K) for this reaction. b) A 100. mL constant volume reaction vessel is loaded with 0.05 mol HBr and heated to 800 K. Calculate the equilibrium constant for this temperature and the partial pressure of Br2 in the equilibrium mixture. Assume Delta standard H and Delta standard S to be independent of temperature.

Correct Answers:

DHo=103.7 kJ/mol, DSo=-21.2 J/K mol, DGo=110.0 kJ/mol, K=5.25 x 10-20

PBr2= PH2=3.78x x 10-3 atm (PHBr is essentially unchanged).

Please show solution

Expert Solution

Since moles of HBr change very small hence assuming its partial pressure remains unchanged.

Please give me better rattings.

Thankyou.

queen_honey_blossom answered 11 months ago

Consider the following reaction: H2(g) +Br2(g) <=> 2HBr(g) Kc=2.0x10^9 at 25C If 0.100 mol H2 and...

Consider the following reaction: H2(g) +Br2(g) <=> 2HBr(g) Kc=2.0x10^9 at 25C If 0.100 mol H2 and 0.200 mol of Br2 were placed in a 10.0L container at 25C, what will the equilibrium concentrations of H2, Br2 and HBr be?

Hydrogen gas reacts with nitrogen gas to form ammonia according to the reaction below. H2 (g)...

Hydrogen gas reacts with nitrogen gas to form ammonia according to the reaction below. H2 (g) + N2 (g) → NH3 (g) a. How many moles of NH3 are produced for every 1 mole of H2? Classify this reaction. b. Suppose 12.2 g of H2 (g) reacts with 48.4 g of N2 (g). Identify the limiting reactant. What is the theoretical yield of the ammonia product in grams ? Show your work. c. What mass (in grams) of the excess...

The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.95 x...

The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.95 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 10.70 atm of HBr is introduced into a sealed container at this temperature.

The reaction H2(g) + Br2(g) 2HBr(g) has Kc = 2.0 x 109 at 25 °C. If...

The reaction H2(g) + Br2(g) 2HBr(g) has Kc = 2.0 x 109 at 25 °C. If 0.100 mol of H2 and 0.100 mol of Br2 were placed in a 10.0 L container and allowed to react, what would all the equilibrium concentrations be at 25 °C?

Consider the chemical reaction: C(s)+H2O(g)→CO(g)+H2(g) How many liters of hydrogen gas are formed from the complete...

Consider the chemical reaction: C(s)+H2O(g)→CO(g)+H2(g) How many liters of hydrogen gas are formed from the complete reaction of 1.16 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and temperature of 319 K. ( ANSWER SHOULD BE IN LITERS ) Express your answer using two significant figures. CH3OH can be synthesized by the reaction: CO(g)+2H2(g)→CH3OH(g) How many liters of H2 gas, measured at 741 mmHg and 88 ∘C, are required to synthesize 0.68...

Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌...

Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H2, I2, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.547 M. [H2]= [I2]= [HI]=

8. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇌ 2 HBr(g) is 2.18×106...

8. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇌ 2 HBr(g) is 2.18×106 at 730°C. Starting 3.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium. the answer is [H2] = [Br2] = 1.81×10-4 M [HBr] = 0.267 M but how and why?

Calculate delta H for the reaction H(g) + Br(g) = HBr(g), given the following information: H2(g)...

Calculate delta H for the reaction H(g) + Br(g) = HBr(g), given the following information: H2(g) + Br2(g) = 2HBr(g) delta H = -72 kJ H2(g) = 2H(g) delta H = +436 kJ Br2(g)= 2Br(g) delta H = +224 kJ

The reaction of nitric oxide (NO(g)) with molecular hydrogen (H2(g)) results in the formation of nitrogen...

The reaction of nitric oxide (NO(g)) with molecular hydrogen (H2(g)) results in the formation of nitrogen and water as follows: 2NO (g) + 2H2(g)...> N2(g) + 2H2O(g) The experimentally determined rate-law expression for this reaction is first order in H2(g) and second order with NO(g). a) Is the reaction above, as written an elementary reaction? b) One potential mechanism for this reaction is as follows: H2(g) + 2NO(g)...> N2O (g) + H2O (g) k1 H2(g) + N2O (g)...> N2(g) +...

Consider this reaction: H2(g) + O2 (g) à H2O (g) &nbsp

Consider this reaction: H2(g) + O2 (g) à H2O (g) dHo = __________ Balance the equation and put the correct number of moles in the equation above. (1 point) Classify the forward reaction as (1) Combustion, (2) Decomposition, (3) Single replacement, (4) Double replacement, (5) Neutralization, (6) Synthesis. Circle the correct answer. (1 point) In this reaction did Hydrogen get oxidized or reduced? Circle the correct answer. (1 point) Based on your answer above is Hydrogen an...

Question