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sweet-ann [11.9K]
3 years ago
15

A + B ->CWhich situation best describes the effect of a limiting reactant?

Chemistry
1 answer:
anygoal [31]3 years ago
7 0

Answer:

The Limiting Reactant is the reactant that when consumed the reaction stops.

Explanation:

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A buffer solution is composed of 4.00 4.00 mol of acid and 3.25 3.25 mol of the conjugate base. If the p K a pKa of the acid is
Reika [66]

<u>Answer:</u> The pH of the buffer is 4.61

<u>Explanation:</u>

To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:

pH=pK_a+\log(\frac{[\text{conjuagate base}]}{[\text{acid}]})

We are given:

pK_a = negative logarithm of acid dissociation constant of weak acid = 4.70

[\text{conjuagate base}]} = moles of conjugate base = 3.25 moles

[\text{acid}]  = Moles of acid = 4.00 moles

pH = ?

Putting values in above equation, we get:

pH=4.70+\log(\frac{3.25}{4.00})\\\\pH=4.61

Hence, the pH of the buffer is 4.61

8 0
3 years ago
What is true about ionic compounds?
bezimeni [28]
It’s D I am pretty sure.
6 0
3 years ago
What is the value for ∆Soreaction for the following reaction, given the standard entropy values? 2H2S(g) + SO2(g) 3Srhombic(s) +
Mademuasel [1]

Answer: \Delta S^{0} for the reaction is -186.75 J/K

Explanation:

Change in entropy (\Delta S^{0}) for the given reaction under standard condition is given by-

\Delta S^{0}= [3\times S_{rhombic}^{0}_{(s)}]+[2\times S_{H_{2}O}^{0}_{(g)}]-[2\times S_{H_{2}S}^{0}_{(g)}]-[1\times S_{SO_{2}}^{0}_{(g)}]

So \Delta S^{0} = [3\times 31.8 J/K.mol]+[2\times 188.825 J/K.mol]-[2\times 205.79 J/K.mol]-[1\times 248.22 J/K.mol] = -186.75 J/K

5 0
3 years ago
Calculate the equilibrium constant at 25 ∘C for the reaction Fe(s)+2Ag+(aq)→Fe2+(aq)+2Ag(s)
Murrr4er [49]

Answer:

1.7 × 10 ^42

Explanation:

Using Nernst equation

E°cell = RT/nF Inq

at equilibrium

Q=K

E°cell  = 0.0257 /n Ink= 0.0592/n log K

Fe2+(aq)+2e−→Fe(s)     E∘= −0.45 V

Ag+aq)+e−→Ag(s)         E∘= 0.80 V

Fe(s)+2Ag+(aq)→Fe2+(aq)+2Ag(s)

balance the reaction

Fe → Fe²⁺ + 2e⁻  reversing for oxidation E° = 0.45 v

2 Ag⁺ +2e⁻ → 2Ag

n = 2 moles  and K = equilibrium constant

E° cell = 0.80 + 0.45 = 1.25 V

E° cell = (0.0592 / n) log K  

substitute the value into the equations and solve for K

(1.25 × 2) / 0.0592  = log K

42.23 = log K

k = 10^ 42.23

K = 1.7 × 10 ^42

8 0
3 years ago
For a particular chemical reaction, the enthalpy of the reactants is -400 kJ. The enthalpy of the products is -390 kJ. The entro
Hunter-Best [27]

Answer:

For a particular chemical reaction, the enthalpy of the reactants is -400 kJ. The enthalpy of the products is -390 kJ. The entropy of the reactants is 0.2 kJ/K. The entropy of the products is 0.3 kJ/K. The temperature of the reaction is 25oC. What can you conclude about this reaction?

It is exergonic

It is endergonic

it is a redox reaction

It is being catalyzed by an enzyme

6 0
2 years ago
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