Reaction quotient (Q) : It is defined as the measurement of the relative amounts of products and reactants present during a reaction at a particular time.

The given balanced chemical reaction is,

$C(s)+H_2O(g)\rightarrow CO(g)+H_2(g)$

The expression for reaction quotient will be :

$Q=\frac{[CO][H_2]}{[H_2O]}$

In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.

Now we have to calculate the concentration of $H_2O,CO\text{ and }H_2$

$\text{Concentration of }H_2O=\frac{\text{Moles of }H_2O}{\text{Volume of solution}}=\frac{13.3mol}{3.25L}=4.09M$

and,

$\text{Concentration of }CO=\frac{\text{Moles of }CO}{\text{Volume of solution}}=\frac{3.40mol}{3.25L}=1.05M$

and,

$\text{Concentration of }H_2=\frac{\text{Moles of }H_2}{\text{Volume of solution}}=\frac{6.30mol}{3.25L}=1.94M$

Now put all the given values in the above expression, we get:

$Q=\frac{(1.05)\times (1.94)}{(4.09)}=0.498$

Thus, the value of reaction quotient Q is, 0.498

3 0

3 years ago

A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 23.0 mL of

Rus_ich [418]

52.0ml of 0.35M CH3COOH : 0.052 L(0.35M) = .0182 mol of CH3COOH.

31.0ml of 0.40M NaOH : .031 L(0.40M) = .0124 mol of NaOH.

After the reaction, .0124 Mol CH3COO- is generated and .058 mol CH3COOH is left un-reacted. The concentration would be 12.4/V and 5.8/V, respectively. Therefore:


pH = -log([H+]) = -log(Ka*[CH3COOH]/[CH3COO-]) 
= -log(1.8x10^-5*5.8/12.4) = 5.07

6 0

3 years ago

What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 5.0? Not

Leni [432]

Answer:

Acetic acid 0,055M and acetate 0,095M.

Explanation:

It is possible to prepare a 0,15M buffer of acetic acid/acetate at pH 5,0 using Henderson-Hasselblach formula, thus:

pH = pka + log₁₀ [A⁻]/[HA] -Where A⁻ is acetate ion and HA is acetic acid-

Replacing:

5,0 = 4,76 + log₁₀ [A⁻]/[HA]

1,7378 = [A⁻]/[HA] (1)

As concentration of buffer is 0,15M, it is possible to write:

[A⁻] + [HA] = 0,15M (2)

Replacing (1) in (2):

1,7378[HA] + [HA] = 0,15M

2,7378[HA] = 0,15M

[HA] = 0,055M

Thus, [A⁻] = 0,095M

That means you need acetic acid 0,055M and acetate 0,095M to obtain the buffer you need.

i hope it helps!

7 0

3 years ago

A reading shows a pressure measurement of 43 in. Hg. What is the equivalent pressure in psi? A. 5.73 psi B. 2223.13 psi C. 26.32

oksian1 [2.3K]

43 inHg = 43 inHg*2.54cm/in = 109.22cmHg * 10 mm/cm = 1092.2 mmHg

14.7 psi = 760 mmHg

1092.2mmHg * 14.7psi / 760 mmHg = 21.13 psi

Answer: option D. 21.13 psi

7 0

3 years ago

Read 2 more answers