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Lostsunrise [7]
3 years ago
7

What is the Molar mass of Na3P

Chemistry
1 answer:
Sedaia [141]3 years ago
6 0

Answer:

99.943071 g/mol

Explanation:

22.98977*3+30.973761

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8_murik_8 [283]

The answer is C. 2 m/s

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Calculate the pH in titration of a weak acid: What is the pH in titration of formic acid (HCHO2, 0.200 M, 100.0 mL) after the ad
ki77a [65]

Answer:

pH = 12.61

Explanation:

First of all, we determine, the milimoles of base:

0.120 M = mmoles / 300 mL

mmoles = 300 mL . 0120 M = 36 mmoles

Now, we determine the milimoles of acid:

0.200 M = mmoles / 100 mL

mmoles = 100 mL . 0.200M = 20 mmoles

This is the neutralization:

HCOOH    +     OH⁻         ⇄        HCOO⁻     +    H₂O

20 mmol       36 mmol             20 mmol

                    16 mmol

We have an excess of OH⁻, the ones from the NaOH and the ones that formed the salt NaHCOO, because this salt has this hydrolisis:

NaHCOO  →  Na⁺  +  HCOO⁻

HCOO⁻  +  H₂O  ⇄   HCOOH  +  OH⁻   Kb →  Kw / Ka = 5.55×10⁻¹¹

These contribution of OH⁻ to the solution is insignificant because the Kb is very small

So:  [OH⁻] =  16 mmol / 400 mL →  0.04 M

- log  [OH⁻]  = pOH →  1.39

pH = 14 - pOH → 12.61

6 0
3 years ago
Nitric oxide (NO) reacts readily with chlorine gas as follows.2 NO(g) + Cl2(g) equilibrium reaction arrow 2 NOCl(g)At 700. K the
Yanka [14]

<u>Answer:</u>

<u>For a:</u> The mixture will need to produce more reactants to reach equilibrium.

<u>For b:</u> The mixture will need to produce more reactants to reach equilibrium.

<u>For c:</u> The mixture will need to produce more products to reach equilibrium.

<u>Explanation</u>:

For the given chemical equation:

2NO(g)+Cl_2(g)\rightleftharpoons 2NOCl(g)

The expression of K_{p} for above equation follows:

K_{p}=\frac{(p_{NOCl})^2}{(p_{NO})^2\times p_{Cl_2}}   .....(1)

We are given:

Value of K_p = 0.26

There are 3 conditions:

  • When K_{p}>Q_p; the reaction is product favored.
  • When K_{p}; the reaction is reactant favored.
  • When K_{p}=Q_p; the reaction is in equilibrium.

For the given options:

  • <u>For a:</u>

We are given:

p_{NOCl}=0.11atm\\p_{NO}=0.16atm\\p_{Cl_2}=0.30atm

Putting values in expression 1, we get:

Q_p=\frac{(0.11)^2}{(0.16)^2\times 0.30}=1.57

As, K_{p}; the reaction is reactant favored

Hence, the mixture will need to produce more reactants to reach equilibrium.

  • <u>For b:</u>

We are given:

p_{NOCl}=0.048atm\\p_{NO}=0.12atm\\p_{Cl_2}=0.10atm

Putting values in expression 1, we get:

Q_p=\frac{(0.048)^2}{(0.12)^2\times 0.10}=1.6

As, K_{p}; the reaction is reactant favored

Hence, the mixture will need to produce more reactants to reach equilibrium.

  • <u>For c:</u>

We are given:

p_{NOCl}=5.20\times 10^{-3}atm\\p_{NO}=0.15atm\\p_{Cl_2}=0.15atm

Putting values in expression 1, we get:

Q_p=\frac{(5.20\times 10^{-3})^2}{(0.15)^2\times 0.15}=0.008

As, K_{p}>Q_p; the reaction is product favored.

Hence, the mixture will need to produce more products to reach equilibrium.

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Moles * Avogadro constant = 5.52 * <span>6.022 x 10^23</span>
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