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Reil [10]
2 years ago
14

What is the mass percentage of Li2CO3

Chemistry
1 answer:
asambeis [7]2 years ago
7 0

Answer: its supposed to be  18.78%.

Explanation:

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Which isotope has the greatest number of protons?
tino4ka555 [31]

Answer:

The isotope with the greatest number of protons is:

  • <u>option D:  Pu-239, with 94 protons</u>

Explanation:

The number of <em>protons</em> is the atomic number and is a unique number for each type of element.

You can tell the number of protons searching the element in a periodic table and reading its atomic number.

Thus, this is how you tell the number of protons or each isotope

Sample       Chemical symbol  Element       atomic number   # of protons

A Pa-238       Pa                         protactinium         91                        91

B U-240         U                          uranium                 92                       92

C Np-238       Np                        neptunium            93                       93

D Pu-239        Pu                        plutonium              94                       94

8 0
3 years ago
I don't know how to solve this​
Misha Larkins [42]

For the first part, use the question M=mol/vol (liters)

To do this, you have the given 1.6 M solution

divide the 360g by the molar mass of ethanol (44.07) to get moles

360/44.07=8.16 mol

so

1.6M = 8.16 mol/x vol

volume: 5.1 Liters

8 0
3 years ago
In a synthesis reaction you start with 1.7L of Hydrogen how many liters of water will be produced?
jolli1 [7]

15.3 litres of water will be produced if we take 1.7 litres of Hydrogen

Explanation:

Let's take a look over synthesis reaction;

H_{2}+ O_{2}<u>                         </u>H_{2}O<u />

<u>Balancing the chemical reaction;</u>

2H_{2} +O_{2}<u>                        </u>2H_{2}O<u />

Thus, 2 moles of hydrogen molecules are required to form 2 moles of water molecules.

<u>Equating the molarity;</u>

<u />\frac{1.7*1}{2*2} = \frac{x*1}{2*18}

           (Since, the molecular mass of hyd and water is 2 and 18 respectively)

x=\frac{1.7*2*18}{2*2}

x= 15.3 litres.

Thus,15.3 L of water will be produced if we take 1.7 litres of Hydrogen in a synthesis reaction.

6 0
3 years ago
What part of the leaf is responsible for absorbing the sun’s energy?
never [62]

Answer:chlorophyll

Explanation:

3 0
2 years ago
CO2(g)+CCl4(g)⇌2COCl2(g) Calculate ΔG for this reaction at 25 ∘C under these conditions: PCO2PCCl4PCOCl2===0.140 atm0.185 atm0.7
padilas [110]

<u>Answer:</u> The \Delta G for the reaction is 54.425 kJ/mol

<u>Explanation:</u>

For the given balanced chemical equation:

CO_2(g)+CCl_4(g)\rightleftharpoons 2COCl_2(g)

We are given:

\Delta G^o_f_{CO_2}=-394.4kJ/mol\\\Delta G^o_f_{CCl_4}=-62.3kJ/mol\\\Delta G^o_f_{COCl_2}=-204.9kJ/mol

To calculate \Delta G^o_{rxn} for the reaction, we use the equation:

\Delta G^o_{rxn}=\sum [n\times \Delta G_f(product)]-\sum [n\times \Delta G_f(reactant)]

For the given equation:

\Delta G^o_{rxn}=[(2\times \Delta G^o_f_{(COCl_2)})]-[(1\times \Delta G^o_f_{(CO_2)})+(1\times \Delta G^o_f_{(CCl_4)})]

Putting values in above equation, we get:

\Delta G^o_{rxn}=[(2\times (-204.9))-((1\times (-394.4))+(1\times (-62.3)))]\\\Delta G^o_{rxn}=46.9kJ=46900J

Conversion factor used = 1 kJ = 1000 J

The expression of K_p for the given reaction:

K_p=\frac{(p_{COCl_2})^2}{p_{CO_2}\times p_{CCl_4}}

We are given:

p_{COCl_2}=0.735atm\\p_{CO_2}=0.140atm\\p_{CCl_4}=0.185atm

Putting values in above equation, we get:

K_p=\frac{(0.735)^2}{0.410\times 0.185}\\\\K_p=20.85

To calculate the gibbs free energy of the reaction, we use the equation:

\Delta G=\Delta G^o+RT\ln K_p

where,

\Delta G = Gibbs' free energy of the reaction = ?

\Delta G^o = Standard gibbs' free energy change of the reaction = 46900 J

R = Gas constant = 8.314J/K mol

T = Temperature = 25^oC=[25+273]K=298K

K_p = equilibrium constant in terms of partial pressure = 20.85

Putting values in above equation, we get:

\Delta G=46900J+(8.314J/K.mol\times 298K\times \ln(20.85))\\\\\Delta G=54425.26J/mol=54.425kJ/mol

Hence, the \Delta G for the reaction is 54.425 kJ/mol

7 0
3 years ago
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