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3 years ago

Which electrolyte is stronger, NaOH or Ca(OH)2? Why?

Chemistry

1 answer:

nataly862011 [7]3 years ago

8 0

Answer:

NaOH

Explanation:

Look at charge Na has +1 charge and Ca has +2 charge after dissociation . Greater charge Stronger lattice. And as we need weak Lattice, so NaoH is stronger base than Ca(OH)2.

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How many hydrogen atoms are in 7.80 mol of ammonium sulfide?

Alexus [3.1K]

The number of hydrogen atoms that are in 7.80 moles of ammonium sulfide are 3.756 x 10^25 atoms

calculation

Step 1: calculate the moles of H in (NH4)2S

since there are 8 atoms of H in (NH4)2S the moles of

H = 8 x7.80 = 62.4 mole

Step 2: use of Avogadro's law constant to determine the number of H atom

that is 1 mole = 6.02 x10^23 atoms

62.4 moles=? atoms

cross multiplication

= [ 62.4 x 6.02 x10^23]/ 1 mole= 3.756 x10^25 atoms

7 0

3 years ago

Read 2 more answers

Explain how they would make solutions of the sulfuric acid at five different concentrations

katrin2010 [14]

The sulfuric acid can be constituted into different concentrations using distilled water as a diluent.

<h3>What is dilution of acid?</h3>

Dilution of acid is defined as the decrease in the concentration of an acid using water.

For sulfuric acid to be diluted, it is slowly added to distilled water using the following guidelines:

Add 150 ml of water to the beaker and add the desired amount of acid. This will give a diluted concentration of the given acid.

Learn more about acid here:

brainly.com/question/25148363

#SPJ1

3 0

1 year ago

Ethanol (C2H5OH) melts a - 144 oC and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kj/mol, and its enthalpy of vapo

hammer [34]

Answer:

For a: The total heat required is 36621.5 J

For b: The total heat required is 58944.5 J

Explanation:

For a:

To calculate the heat required at different temperature, we use the equation:

$q=mc\Delta T$ .........(1)

where,

q = heat absorbed

m = mass of substance

$c$ = specific heat capacity of substance

$\Delta T$ = change in temperature

To calculate the amount of heat required at same temperature, we use the equation:

$q=m\times \Delta H$ ........(2)

where,

q = heat absorbed

m = mass of substance

$\Delta H$ = enthalpy of the reaction

The processes involved in the given problem are:

$1.)C_2H_5OH(l)(35^oC)\rightarrow C_2H_5OH(l)(78^oC)\\2.)C_2H_5OH(l)(78^oC)\rightarrow C_2H_5OH(g)(78^oC)$

For process 1:

We are given:

Change in temperature remains the same.

$m=42.0g\\c_l=2.3J/g.K\\T_2=78^oC\\T_1=35^oC\\\Delta T=[T_2-T_1]=[78-35]^oC=43^oC=43K$

Putting values in equation 1, we get:

$q_1=42.0g\times 2.3J/g.K\times 43K\\\\q_1=4153.8J$

For process 2:

We are given:

Conversion factor: 1 kJ = 1000 J

Molar mass of ethanol = 46 g/mol

$m=42.0g\\\Delta H_{vap}=38.56kJ/mol=\frac{35.56kJ}{1mol}\times (\frac{1000J}{1kJ})\times (\frac{1}{46g/mol})=773.04J/g$

Putting values in equation 2, we get:

$q_2=42.0g\times 773.04J/g\\\\q_2=32467.7J$

Total heat required = $[q_1+q_2]$

Total heat required = $[4153.8J+32467.7J]=36621.5J$

Hence, the total heat required is 36621.5 J

For b:

The processes involved in the given problem are:

$1.)C_2H_5OH(s)(-155^oC)\rightarrow C_2H_5OH(s)(-144^oC)\\2.)C_2H_5OH(s)(-144^oC)\rightarrow C_2H_5OH(l)(-144^oC)\\3.)C_2H_5OH(l)(-144^oC)\rightarrow C_2H_5OH(l)(78^oC)\\4.)C_2H_5OH(l)(78^oC)\rightarrow C_2H_5OH(g)(78^oC)$