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3 years ago

How should I write balanced net ionic equation for this reaction?

Chemistry

1 answer:

Maksim231197 [3]3 years ago

3 0

Answer:

Explanation:

Assumptions

They would ionize completely, or you must assume that.
The volumes must be the same as well.
0.11M Cu(NO3)2 ===> 0.11MCu2+ + 0.22 NO3-

Note

The concentrations would merely add. All things change if the assumptions I've made are not true.

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1.Which statement best describes scientific laws

gtnhenbr [62]

In a way, all of the answers could be argued for (for example: in the first option: if the scientists' opinions are understood to be "informed understanding of the causes of events"), but one of the options is the best:
Scientific laws describe specific relationships in nature without offering
an explanation.

The reason why I think this is true is that many laws are phased too short and too concise to provide comprehensive explanations, instead they describe the relationships that must hold.

One of the options is pplain false:
Scientific laws explain why natural events occur. -"Scientific laws were theories that have been tested, proven, and adopted as laws." - since they are not adopted as laws.

6 0

3 years ago

4. When 1.00 L of 1.00 M Ba(NO3)2 solution at 25.0˚C is mixed with 1.00 L of 1.00 M Na2SO4 solution at 25.0˚C in a calorimeter,

myrzilka [38]

Answer:

The final temperature of the mixture is 28.11 °C

Explanation:

Step 1: Data given

Volume of 1.00 M Ba(NO3)2 = 1.00 L

Temperature = 25.0 °C

Volume of 1.00 M Na2SO4 = 1.00 L

enthalpy change is – 26 kJ per mol BaSO4

The specific heat of water is 4.18 J/g ·˚C

the density of water is 1.00 g/mL

Step 2: The balanced equation

Ba(NO3)2(aq) + Na2SO4(aq) → 2NaNO3(aq) + BaSO4(s)

Step 3: Calculate the total volume

Total volume = 1.00 L + 1.00 L = 2.00 L = 2000 mL

Step 4: Calculate mass

Mass = volume * density

Mass = 2000 mL * 1g/mL

Mass = 2000 grams

Step 5: Calculate moles BaSO4 formed

For 1 mol Ba(NO3)2 we need 1 mol Na2SO4 to produce 1 mol BaSO4

There is no limiting reactant, both Ba(NO3)2 and Na2SO4 will be completely be consumed (1 mol). We'll have 1.0 mol of BaSO4 produced.

Step 6: Calculate Q

Q = - ΔH

ΔH is negative so the reaction is exothermic, what means the temperature increases

Q is always positive, so Q = 26kJ = 26000 J

Step 6: Calculate the heat transfer

Q= m*c*ΔT

⇒with Q = the heat transfer = TO BE DETERMINED

⇒with m =the mass of the solution = 2000 grams

⇒with c= the specific heat of the solution = 4.18 J/g°C

⇒with ΔT = the change of temperature = T2 - T1 = T2 - 25.0

26000 = 2000 * 4.18 * (T2 - 25.0 °C)

3.11 = T2 - 25.0 °C

T2 = 25.0 + 3.11 °C

T2 = 28.11 °C

The final temperature of the mixture is 28.11 °C

7 0

3 years ago

The acid-dissociation constant of hydrocyanic acid (hcn) at 25.0 °c is 4.9 ⋅ 10−10. what is the ph of an aqueous solution of 0.0

vodomira [7]

According to the reaction equation:

and by using ICE table:

CN- + H2O ↔ HCN + OH-

initial 0.08 0 0

change -X +X +X

Equ (0.08-X) X X

so from the equilibrium equation, we can get Ka expression

when Ka = [HCN] [OH-]/[CN-]

when Ka = Kw/Kb

= (1 x 10^-14) / (4.9 x 10^-10)

= 2 x 10^-5

So, by substitution:

2 x 10^-5 = X^2 / (0.08 - X)

X= 0.0013

∴ [OH] = X = 0.0013

∴ POH = -㏒[OH]

= -㏒0.0013

= 2.886

∴ PH = 14 - POH

= 14 - 2.886 = 11.11

5 0

3 years ago

Consider the steps in coal gasification: C(coal) + H2O(g) → CO(g) + H2(g) ΔH°rxn = 129.7 kJ CO(g) + H2O(g) → CO2(g) + H2(g) ΔH°r

Volgvan

Answer:

The answer to your question is ΔHrxn = 0 kJ

Explanation:

Process

1.- Multiply Equation 1 by 2

2C(coal) + 2H₂O ⇒ 2CO (g) + 2H₂ ΔH rxn = 259.4 kJ

2.- Sum equation 2

CO(g) + H₂O ⇒ CO₂ (g) + H₂ (g) ΔHrxn = -41 kJ

Result

2C + 3H₂O + CO ⇒ 2CO + 3H₂ + CO₂ ΔHrxn = 218.4 kJ

Simplification

2C + 3H₂O ⇒ CO + 3H₂ + CO₂

3.- Sum equation 3

CO(g) + 3H₂ (g) ⇒ CH₄ (g) + H₂O (g) ΔHrxn = -218.4 kJ

Result

2C + 3H₂O + 3H₂ + CO ⇒ CO + 3H₂ + CO₂ + CH₄ + H₂O

Simplification

2C + 2H₂O ⇒ CO₂ + CH₄ ΔHrxn = 0 kJ

4 0

3 years ago

The heat combustion of glucose (C6H12O6) is desrcribed by the process:

spayn [35]

Answer:

a) Equilibrium will shift to the left i.e. reactants

b) K will increase with increase in temperature

Explanation:

The given reaction is:

C6H12O6 + 6 O2 ↔ 6 CO2 + 6 H2O ΔH = -2816 kJ/mol

a) As per Le Chatelier's principle, for a reaction at equilibrium any changes in temperature, pressure or concentration will shift the equilibrium in a direction so as to undo the effect of the induced change.

The given reaction is exothermic (since ΔH is negative) i.e. it accompanied by the release of heat and hence an increase in temperature. Therefore, if the temperature is increased the equilibrium will shift in the opposite direction i.e. towards the left or towards the reactants.

b) The equilibrium constant (K) and temperature T are related via the Van't Hoff equation:

$[ln\frac{K2}{K1}=\frac{-\Delta H}{R}[\frac{1}{T2}-\frac{1}{T1}]$

In the given reaction, ΔH is negative and the condition is T2>T1

Therefore, K2 > K1

The value of equilibrium constant will increase with increase in temperature

8 0

3 years ago