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 Kc = 64 at 700 K?
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
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
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 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 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 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 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 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 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 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?