Question 1

At equilibrium, a 1.00 L vessel contains 0.0430 mol of , 0.0620 mol of , and 0.358 mole of . The system is represented by the following equation:

H_₂(g)+ I₂ (g) $⇌$ 2HI (g)

Which of the following is closest to the value of the equilibrium constant, $K_{eq}$ , for this reaction?

Accepted Answer

48.1

Answer

269

Answer

134

Answer

0.0208

Question 2

Nitrosyl bromide decomposes according to the following equation.

2NOBr (g) $⇌$ 2NO (g) + Br₂ (g)

A 0.64 mol sample of NOBr is placed in an evacuated 1.00 L flask. After the system comes to equilibrium, the flask contains 0.46 mol NOBr . What are the concentrations of NO and Br₂in the flask at equilibrium?

Accepted Answer

A

Answer

D

Answer

C

Answer

B

Question 3

A system is described as follows.

2NaHCO₃ (s) $⇌$ Na₂CO₃ (s) + CO₂ (g) + H₂O (g)

What is the equilibrium expression for this system?

Accepted Answer

$\mathrm{\ K_{eq}}$ = [CO₂][H₂O]

Answer

$\mathrm{\ K_{eq}}$

Answer

$\mathrm{\ K_{eq}}$ = [CO₂]

Answer

$\mathrm{\ K_{eq}}$ $=\frac{1}{\left[CO_2\right]\left[H_2O\right]}$

Question 4

The equation for the autoionisation of water is shown

2H₂O (l) $⇌$ H₃O⁺ (aq) + OH^- (aq)

At 50°C the water ionisation constant, $K_{eq}$ , 5.5x10^-14 is .

What is the pH of water at 50°C?

Accepted Answer

6.63

Answer

6.93

Answer

5.50

Answer

7.00

Question 5

A student makes a solution with a final volume of 200 mL by mixing 100 mL of 0.0500 mol L ¯¹ barium nitrate solution with 100 mL of 0.100 mol L ¯¹ sodium hydroxide solution. Which option correctly identifies if a precipitate will form under these conditions and the reason?

Accepted Answer

A precipitate will NOT form because $Q\ <\ K\ _{sp}$

Answer

A precipitate WILL form because $Q\ <\ K\ _{sp}$

Answer

A precipitate WILL form because $Q\ <\ K\ _{sp}$

Answer

A precipitate will NOT form because $Q\ <\ K\ _{sp}$

Question 6

Accepted Answer

Related quizzes

Related quizzes