Consider the following reaction:

2 answers:

7 0

Equation: NH4HS(s) <=> NH3 (g) + H2S(g)

Kc = [NH3]eq[H2S]eq; where eq subscripts are used to indicate that those are the concentrations at equilibrium

Kc= 0.272 * 0.365 =0.09928

posledela3 years ago

4 0

Answer : The equilibrium constant is, $9.928\times 10^{-2}$

Solution : Given,

Equilibrium concentration of $NH_3$ = 0.272 M

Equilibrium concentration of $H_2S$ = 0.365 M

The given balanced equilibrium reaction is,

$NH_4HS(s)\rightleftharpoons NH_3(g)+H_2S(g)$

The expression for equilibrium constant will be,

$K_c=\frac{[NH_3][H_2S]}{[NH_4HS]}$

Now put all the given values in this formula, we get value of equilibrium constant.

$K_c=\frac{(0.272)\times (0.365)}{1}$

$K_c=0.09928=9.928\times 10^{-2}$

Therefore, the equilibrium constant is, $9.928\times 10^{-2}$

You might be interested in

Your patient gets a prescription for 62.5 mcg (micrograms, mg) of digoxin in liquid form. The label reads 0.0250 mg/mL. How many

blsea [12.9K]

Answer:

2.5 militers (mL) of digoxin solution

Explanation:

if 1 microgram = 0.001 miligram

then 62.5 micrograms = X miligrams

X = (62.5 × 0.001) / 1 = 0.0625 miligrams

the we calculate the number of militers of digoxin needed by the patient:

if we have 0.0250 miligrams of digoxin in 1 mililiter of solution

then we have 0.0625 miligrams of digoxin in X mililiters of solution

X = (0.0625 × 1) / 0.0250 = 2.5 militers (mL) of digoxin solution

4 0

4 years ago

The combustion of propane may be described by the chemical equation C 3 H 8 ( g ) + 5 O 2 ( g ) ⟶ 3 CO 2 ( g ) + 4 H 2 O ( g ) C

Kipish [7]

Answer: 72 grams of $O_2(g)$ are needed to completely burn 19.7 g $C_3H_8(g)$

Explanation:

According to avogadro's law, 1 mole of every substance weighs equal to molecular mass and contains avogadro's number $6.023\times 10^{23}$ of particles.