All categories

3 years ago

How many moles of silver chloride, produced from 100 g of silver nitrate reacting with barium chloride BaCl2?

Chemistry

1 answer:

Dmitrij [34]3 years ago

7 0

Answer:

Equation of Reaction

2AgNO3 + BaCl2 === 2AgCl + Ba(NO3)2

Molar Mass of AgNO3 = 170g/mol

Moles of reacting AgNO3 = 100g/170gmol-¹

=0.588moles of AgNO3

From the equation of reaction...2moles of AgNO3 reacts to Produce 2Moles of Silver Chloride

So Their ratio is 2:2.

This means that 0.588Moles of AgCl Will be produced too.

ANSWER...0.588MOLES OF AgCl WILL BE PRODUCED.

You might be interested in

What is the molarity of a potassium triiodide solution, KI3(aq), if 30.00 mL of the solution is required to completely react wit

vfiekz [6]

Answer:

The molarity is 0.203 M

Explanation:

Using the formula C(oxi) x V(oxi) / [C(red) x V(red)] = N(oxi) / N(red)

Where oxi and red means reducing agent and oxidising agent respectively.

C = Concentration, V = Volume and N = number of moles.

C(oxi) = 0.5 M

V(oxi) = mL

C(red) = ?

V(red) = 30mL

Equation of reaction = 2K2S2O3 + KI3 = K2S4O6 + 3KI

so N(red) = 1 , N(oxi) = 2

from the equation above,

C(red) = 0.5 x 25 x 1 / (2 x 30)

= 0.203 M.

3 0

3 years ago

The radii of the lithium and magnesium ions are 76 pm and 72 pm, respectively. which compound has stronger ionic attraction, lit

quester [9]

From the Born–Landé equation the lattice energy U ∝ (Z+ × Z-) / (r+ + r-) where Z+ and Z- are the charges on the cation and anion, respectively; r+ and r- are radii of the cation and anion, respectively.

The Z+×Z- term dominates. MgO has 2×2 (4) so it will have the higher U than Li2O Z+ × Z- = 2.
You only consider (r+ + r-) term when the Z+×Z- term is the same; smallest the (r+ + r-), the larger is the U.
U(MgO) = 3795 kJ mol^-1
U(Li2O) = 2799 kJ mol^-1

MgO has larger.

6 0

3 years ago

Suppose you have 100 grams of radioactive plutonium-239 with a half-life of 24,000 years. how many grams of plutonium-239 will r

Alexandra [31]

To solve this problem, let us first calculate for the rate constant k using the half life formula:

t1/2 = ln 2 / k

where t1/2 = half life period = 24,000 years, therefore k is:

k = ln 2 / 24,000

k = 2.89 x 10^-5 / yr

Now we use the rate equation:

A = Ao e^(-k t)

where,

A = mass of Plutonium-239 after number of years

Ao = initial mass of Plutonium-239

t = number of years

A. t = 12,000 years, find A

A = 100g e^(- 2.89 x 10^-5 * 12,000)

A = 70.7 g

B. t = 24,000 years, find A

A = 100g e^(- 2.89 x 10^-5 * 24,000)

A = 50 g

C. t = 96,000 years, find A

A = 100g e^(- 2.89 x 10^-5 * 96,000)

A = 6.24 g

5 0

3 years ago

1 lb of CO2 occupies 0.6 ft^3 at a pressure of 200 psi. Determine the temperature of the system.

Anarel [89]

Answer: The temperature of the system is 273 K

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of carbon dioxide = 1 lb = 453.6 g (Conversion factor: 1 lb = 453.6 g)

Molar mass of carbon dioxide = 44 g/mol

Putting values in above equation, we get:

$\text{Moles of carbon dioxide}=\frac{453.6g}{44g/mol}=10.31mol$

To calculate the temperature of gas, we use the equation given by ideal gas equation:

PV = nRT

where,

P = Pressure of carbon dioxide = 200 psia = 13.6 atm (Conversion factor: 1 psia = 0.068 atm)

V = Volume of carbon dioxide = $0.6ft^3=16.992L$ (Conversion factor: $1ft^3=28.32L$ )

n = number of moles of carbon dioxide = 10.31 mol

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature of the system = ?

Putting values in above equation, we get:

$13.6atm\times 16.992L=10.31mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times T\\\\T=273K$

Hence, the temperature of the system is 273 K

8 0

4 years ago

3. Write DISSOCIATION or IONIZATION equations for the following chemicals:

Romashka [77]

Answer:

a) HNO3 -> H+ + NO3- disassociation of Nitric Acid; to yield a Nitrate ion and a Proton, H+, or as a Hydronium ion H3O+

b) H2S04 -> Disassociation of Sulfuric Acid; simple way- 2H+ + SO4- -

c) H2S hydrogen sulphide in water is an acid; thus H+ HS- disassociation.

d) NaOH -> dissociation of Na+ + OH-; this is complete; sodium hydroxide is deliquescent, meaning it will draw water - EVEN from the air! Strong Base

e) Na2CO3 -> 2Na+ CO3- - Ionization of sodium carbonate - a salt

f) Na2S04 -> 2Na+ + SO4 - - ionization of sodium sulphate - a salt

g) NaCl -> Na+ + Cl- ionization of the salt, Sodium Chloride

Explanation:

Salts ionize at different rates; acids or bases dissociate; these are mostly strong acids and NaOH, a strong base.

8 0

3 years ago