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IrinaVladis [17]
3 years ago
8

a 3.81 g sample of NaHCO3 was completely decomposed. After decomposition, Na2CO3 had mass of 2.86g. Determine mass of H2CO3 prod

uced.
Chemistry
1 answer:
qaws [65]3 years ago
8 0

Answer:

1.67g H2CO3 are produced

Explanation:

Based on the reaction:

2NaHCO3 → Na2CO3 + H2CO3

<em>2 moles of NaHCO3 produce 1 mole of Na2CO3 and 1 mole of H2CO3</em>

To solve this question we need to find the moles of Na2CO3 = Moles of H2CO3. With their moles we can find the mass of H2CO3 as follows:

<em>Moles Na2CO3 -Molar mass: 105.99g/mol-</em>

2.86g Na2CO3 * (1mol/105.99g) = 0.02698 moles Na2CO3 = Moles H2CO3

<em>Mass H2CO3 -Molar mass: 62.03g/mol-</em>

0.02698 moles  * (62.03g/mol) =

<h3>1.67g H2CO3 are produced</h3>

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DochEvi [55]

Answer:

During a total lunar eclipse, the Earth lies directly between the sun and the moon, causing the Earth to cast its shadow on the moon.

Explanation:

4 0
3 years ago
PH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoioniz
ruslelena [56]

Answer:

  • A) pH = 2.42
  • B) pH = 12.00

Explanation:

<em>The dissolution of HCl is  HCl → H⁺ + Cl⁻</em>

  • To solve part A) we need to calculate the concentration of H⁺, to do that we need the moles of H⁺ and the volume.

The problem gives us V=2.5 L, and the moles can be calculated using the molecular weight of HCl, 36.46 g/mol:

0.35g_{HCl}*\frac{1mol_{HCl}}{36.46g_{HCl}} *\frac{1molH^{+}}{1mol HCl} = 9.60*10⁻³ mol H⁺

So the concentration of H⁺ is

[H⁺] = 9.60*10⁻³ mol / 2.5 L = 3.84 * 10⁻³ M

pH = -log [H⁺] = -log (3.84 * 10⁻³) = 2.42

  • <em>The dissolution of NaOH is  NaOH → Na⁺ + OH⁻</em>
  • Now we calculate [OH⁻], we already know that V = 2.0 L, and a similar process is used to calculate the moles of OH⁻, keeping in mind the molecular weight of NaOH, 40 g/mol:

0.80g_{NaOH}*\frac{1mol_{NaOH}}{40g_{NaOH}} *\frac{1molOH^{-}}{1mol NaOH}= 0.02 mol OH⁻

[OH⁻] = 0.02 mol / 2.0 L = 0.01

pOH = -log [OH⁻] = -log (0.01) = 2.00

With the pOH, we can calculate the pH:

pH + pOH = 14.00

pH + 2.00 = 14.00

pH = 12.00

5 0
3 years ago
Then if I have 210.1 g barium chloride with 45g potassium...how many grams of potassium chloride will I produce?
Katarina [22]

Answer:

  85.8 g

Explanation:

The molar mass of BaCl₂ is 208.233 g/mol, so 210.1 g is about ...

  210.1/208.233 ≈ 1.009 mol

The molar mass of K is about 39.089 g/mol, so 45 g is about ...

  45/39.089 ≈ 1.1509 mol

The balanced equation seems to be ...

  BaCl₂ + 2K  ↔ 2KCl + Ba

This reaction requires 2 moles of potassium for each mole of barium chloride, so the available potassium limits the reaction. The result is as many moles of potassium chloride as there are moles of potassium.

The 1.1509 moles of KCl, at 74.551 g/mol will have a mass of about 85.8 g.

The reaction produces 85.8 g of KCl.

8 0
3 years ago
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Is the caffeine molecule polar or non polar?
malfutka [58]
The caffeine molecule is a polar molecule.
7 0
4 years ago
What is the volume of a gas balloon filled with 4.0 moles of tha gas, when the barometer reads pressure of 780 Torr and temperat
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Answer:

V = 96.61 L

Explanation:

Given data:

Number of moles = 4.0 mol

Pressure = 780 torr (780/760 = 1.03 atm)

Temperature = 30°C

Volume of gas = ?

Solution:

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

Now we will convert the temperature.

30+273 = 303 K

1.03 atm × V = 4.0 mol × 0.0821 atm.L/ mol.K  × 303 K

V = 99.505 atm.L / 1.03 atm

V = 96.61 L

5 0
3 years ago
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