0.05 mol H2 (g) and and 0.05 mol Br2 (g) are placed together in a 5.0...

0.05 mol H₂ (g) and and 0.05 mol Br₂ (g) are placed together in a 5.0 L flask and
heated to 700 K. What is the concentration of each substance in the flask at
equilibrium if K_c = 64 at 700 K?

H₂ (g) + Br₂ (g) ⇔ 2HBr(g)

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

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?

A mixture of 1.374 g of H2 and 70.31 g of Br2 is heated in a...

A mixture of 1.374 g of H2 and 70.31 g of Br2 is heated in a 2.00 L vessel at 700 K . These substances react as follows: H2(g)+Br2(g)⇌2HBr(g) At equilibrium the vessel is found to contain 0.566 g of H2. 1A) Calculate the equilibrium concentration of Br2 1B) Calculate Kc. 1C) Calculate the equilibrium constant Kp for this reaction, given the following information (at 299 K ): 2NO(g)+Br2(g)⇌2NOBr(g) Kc=1.8 2NO(g)⇌N2(g)+O2(g) Kc=2.3×10^30 Thank you in advance!

A mixture of 1.397 g of H2 and 70.76 g of Br2 is heated in a...

A mixture of 1.397 g of H2 and 70.76 g of Br2 is heated in a 2.00 L vessel at 700. K. These substances react according to H2(g) + Br2(g) ↔ 2 HBr(g). At equilibrium the vessel is found to contain 0.592 g of H2. (a) Calculate the equilibrium concentrations of H2, Br2, and HBr. (b) Calculate Kc.

A.) Initially, 1.0 mol of H2 and 2.0 mol of I2 are placed into a 10.0...

A.) Initially, 1.0 mol of H2 and 2.0 mol of I2 are placed into a 10.0 L reaction flask. When equilibrium was established, the [HI] was 0.080 mol/L. Find the equilibrium concentrations of H2 and I2 and evaluate Kc for the following reaction: H2 (g)+ I2 (g) <--> 2HI (g) B.) The equilibrium constant for the reaction above is 45.0 at 490 C. What is the equilibrium concentration of each species if 1.0 mol of HI were put in a...

At a certain temperature, 0.4011 mol of N2 and 1.581 mol of H2 are placed in...

At a certain temperature, 0.4011 mol of N2 and 1.581 mol of H2 are placed in a 1.50L container. N2(g) + 3H2(g) −⇀↽− 2NH3(g) At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Kc.

A mixture of 0.750 mol H2 and 0.750 mol I2 was placed in a 1.00 L...

A mixture of 0.750 mol H2 and 0.750 mol I2 was placed in a 1.00 L flask at 430°C. The equilibrium constant Kc for the reaction is 54.3 at this temperature. Calculate the concentration of H2, I2, and HI at equilibrium. H2 + I2 ⇌ 2 HI

A sample of gas contains 0.1000 mol of HCl(g) and 5.000×10-2 mol of Br2(g) and occupies...

A sample of gas contains 0.1000 mol of HCl(g) and 5.000×10-2 mol of Br2(g) and occupies a volume of 4.79 L. The following reaction takes place: 2HCl(g) + Br2(g)2HBr(g) + Cl2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. A sample of gas contains 0.1800 mol of HCl(g) and 9.000×10-2 mol of Br2(g) and occupies a volume of 9.74 L. The following reaction takes place: 2HCl(g) + Br2(g)2HBr(g)...

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?

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?

Subjects