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irinina [24]
3 years ago
8

Please help with word equations?

Chemistry
1 answer:
Delvig [45]3 years ago
7 0
For the answer to the questions above, 

a) Ag2CO3(s) => Ag2O(s)+CO2(g) 

<span>b) Cl2(g)+2(KI)(aq) => I2(s)+2(KCl)(aq) (coefficients are for balanced equation) </span>
<span>net ionic is Cl2(g)+2I- => I2(s)+2Cl-(aq) </span>

<span>c) I2(s)+3(Cl2)(g)=>2(ICl3)
</span>I hope I helped you with your problem
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If the reaction N2 (g) + 3 H2 (g) --&gt; 2 NH3 (g) has the concentrations 1.1 M for nitrogen, 0.75 M for hydrogen and 0.25 M fo
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<u>Answer:</u> The value of K_c is 0.136 and is reactant favored.

<u>Explanation:</u>

Equilibrium constant in terms of concentration is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as K_{c}

For the chemical reaction between carbon monoxide and hydrogen follows the equation:

N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)

The expression for the K_{c} is given as:

K_{c}=\frac{[NH_3]^2}{[N_2][H_2]^3}

We are given:

[NH_3]=0.25M

[H_2]=0.75M

[N_2]=1.1M

Putting values in above equation, we get:

K_c=\frac{(0.25)^2}{1.1\times (0.75)^3}

K_c=0.135

There are 3 conditions:

  • When K_{c}>1; the reaction is product favored.
  • When K_{c}; the reaction is reactant favored.
  • When K_{c}=1; the reaction is in equilibrium.

For the given reaction, the value of K_c is less than 1. Thus, the reaction is reactant favored.

Hence, the value of K_c is 0.136 and is reactant favored.

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If you know your acid concentration is .650 M and you used 15.00 mL, what was the concentration of the base if you needed 35.5 m
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Since the name of the acid (and the equation) is not given, you must assume that it is a 1:1 ratio. Use equation: volume of acid x molarity of acid = volume of base x molarity of base (when the ratio is 1:1).

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