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2 years ago

Nh4i(aq)+koh(aq)→ express your answer as a chemical equation. identify all of the phases in your answer.

2 answers:

5 0

NH4I (aq) + KOH (aq) in chemical equation gives

NH4I (aq) + KOH (aq) = KI (aq) + H2O(l) + NH3 (l)

Ki is in aqueous state H2o is in liquid state while NH3 is in liquid state

from the equation above 1 mole of NH4I (aq) react with 1 mole of KOH(aq) to form 1mole of KI(aq) , 1mole of H2O(l) and 1 Mole of NH3(l)

Norma-Jean [14]2 years ago

4 0

Answer:

NH4I(aq) + KOH(aq) -------->KI(aq) + NH3(g) + H2O(l)

Explanation:

NH4I(aq) + KOH(aq) -------->KI(aq) + NH3(g) + H2O(l)

This is a reaction of aqueous ammonium iodide and aqueous potassium hydroxide to yield aqueous potassium iodide, gaseous ammonia and liquid water as shown above.

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The French chemists, Pierre L. Dulong and Alexis T. Petit, noted in 1819 that the molar heat capacity of many solids at ordinary

natita [175]

The empirical formula of the compound : <u><em>RbO₂</em></u>

<h3>Further explanation</h3>

Dulong and Petit's rule's rule, which says that the molar heat capacity, Cp, of a solid can be expressed as

$\large{\boxed{\bold{Cp=N(3R)}}$

Where N is the number of atoms per formula unit and R is the universal gas constant

While the value of R is:

R = 8.3144621 J / K · mol

then:

3R = 24.94 J / K · mol

Heat capactiy per gram of a compound containing rubidium and oxygen is 0.64 J · K⁻¹ · g⁻¹

We try the possible empirical formula from the composition of Rb and O

Rb₂O

So the number of atoms: 3 (Rb = 2 atoms, O = 1 atom)

Then the value of the Cp:

Molar mass Rb₂O = 2.85.5 + 1.16 = 187 g/mol

$\displaystyle Cp=N(3R)\\\\0.64=\frac{3.24.94}{187}\\\\0.64\neq0.4$

Then this empirical formula Rb₂O is not appropriate

RbO₂

So the number of atoms: 3 (Rb = 1 atom, O = 2 atoms)

Then the value of the Cp:

Molar mass RbO₂ = 1.85.5 + 2.16 = 117.5 g / mol

$\displaystyle Cp=N(3R)\\\\0.64=\frac{3.24.94}{117.5}\\\\0.64=0.64$

Then this empirical formula RbO₂ is appropriate

<h3>Learn more </h3>

chemical bond

brainly.com/question/5008811

ionic bonding

brainly.com/question/1603987

electron dots

brainly.com/question/6085185

Keywords: an empirical formula,compound, gas constant, Dulong and Petit's rule,the molar heat capacity

#LearnWithBrainly

7 0

2 years ago

Determine the PH at the point in the titration of 40.0ml of 0.200M HC4H7o2 with 0.100 M Sr(OH)2 after 100ml of the strong base h

Dmitriy789 [7]

Answer:

Check the explanation

Explanation:

Mols HC4H7O2 = (volume in L)*(molarity) = (40.0 mL)*(0.200 M)

= (40.0 mL)*(1 L)/(1000 mL)*(0.200 M)

= 8.00*10-3 mol.

Mols Sr(OH)2 corresponding to 10.0 mL of 0.100 M solution =

(volume in L)*(molarity)

= (10.0 mL)*(0.100 M)

= (10.0 mL)*(1 L)/(1000 mL)*(0.100 M)

= 1.00*10-3 mol.

Consider the ionization of Sr(OH)2 as below.

Sr(OH)2 (aq) ----------> Sr2+ (aq) + 2 OH- (aq)

As per the stoichiometric equation,

1 mol Sr(OH)2 = 2 mols OH-.

Therefore,

0.0010 mol Sr(OH)2 = [0.0010 mol Sr(OH)2]*(2 mols OH-)/[1 mole Sr(OH)2]

= 0.0020 mol

= 2.00*10-3 mol

Set up the ICE charts as below.

HC4H7O2 (aq) + OH- (aq) ------------> H2O (l) + C4H7O2- (aq)

Before (mol) 8.00*10-3 2.00*10-3 - -

Change (mol) -2.00*10-3 -2.00*10-3 - +2.00*10-3

After (mol) 6.00*10-3 0 - 2.00*10-3

The change in a pure substance, e.g., H2O is not considered in an acid-base reaction.

Volume of the solution = (40.0 + 10.0) mL = 50.0 mL = (50.0 mL)*(1 L)/(1000 mL) = 0.05 L.

The initial concentrations are obtained by dividing the numbers of moles by the volume, 0.05 L.

Set up the ICE charts as below.

HC4H7O2 (aq) + OH- (aq) ------------> H2O (l) + C4H7O2- (aq)

Initial (M) 0.160 0.0400 - -

Change (M) -0.0400 -0.0400 - +0.0400

Equilibrium (M) 0.120 0 - 0.0400

The acid-ionization constant is written as

Ka = [H3O+][C4H7O2-]/[HC4H7O2] = 1.5*10-5

Plug in the known values and get

Ka = [H3O+]*(0.0400)/(0.120) = 1.5*10-5

======> [H3O+] = (1.5*10-5)*(0.120)/(0.0400) (ignore units)

======> [H3O+] = 4.5*10-5

The proton concentration of the solution is 4.5*10-5 M.

pH = -log (4.5*10-5 M)

= 4.346

≈ 4.35 (ans).

8 0

1 year ago

The table above summarizes data given to a student to evaluate the type of change that took place when substance X was mixed wit

Tamiku [17]

The question is incomplete, the complete question is;

The table above summarizes data given to a student to evaluate the type of change that took place when substance X was mixed with water. The student claimed that the data did not provide enough evidence to determine whether a chemical or physical change took place and that additional tests were needed. Which of the following identifies the best way to gather evidence to support the type of change that occurred when water and Xwere mixed?

A. Measuring the melting point of the mixture of water and X

B. Adding another substance to the mixture of water and X to see whether a solid forms

C Measuring and comparing the masses of the water, X, and the mixture of water and X

D Measuring the electrical conductivities of X and the mixture of water and X

Answer:

D Measuring the electrical conductivities of X and the mixture of water and X

Explanation:

Unfortunately, I am unable to reproduce the table here. However, from the table, the temperature of the of the mixture of the solid X and water was 101.6°C. This is above the boiling point of water and way below the temperature of the solid X.

This goes a long way to suggest that there was some kind of interaction between the water and X which accounted for the observed temperature of the system of X in water.

The only way we can be able to confirm if X actually dissolved in water is to measure the conductivity of the water. dissolved solids increase the conductivity of water.

6 0

1 year ago

Calculate the grams of so2 gas present at stp in a 5.9 l container. (r = 0.0821 l·atm/k·mol)

Neko [114]

There is an exact value for the standard volume at standard conditions of 1 atm and 273 K. This standard volume for any ideal gas is 22.4 L/mol. Thus,

Moles SO₂ = 5.9 L * 1 mol/22.4 L = 0.263 mol

The molar mass for SO₂ is 64.066 g/mol. So, the mass is:

Mass = 0.263 mol * 64.066 g/mol = <em>16.87 g SO₂</em>

6 0

2 years ago

How many known elements have atoms, in their ground-state, with valence electrons whose quantum numbers are n = 5 and l = 1?a. 3

Goshia [24]

Answer:

c. 6.

Explanation:

Looking at the description given in the question, the elements involved must belong to the p- block of the periodic table and must be in period 5. They also must possess valence electrons in the 5p- orbital.

Now if we look at the p- block of period 5, the following elements satisfy these requirements; Sr, In, Sn, Sb, Te and I.

Hence there are six of such elements.

7 0

1 year ago