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Volgvan
3 years ago
10

What is tissue onion make of?

Chemistry
2 answers:
d1i1m1o1n [39]3 years ago
5 0
Tissue onion is made out of layers, each layer is separated by a thin skin or membrane
soldier1979 [14.2K]3 years ago
4 0
Tissue onion is made of layers, each separated by a thin skin or membrane

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2-A gas sample is found to contain 39.10% carbon, 7.67% hydrogen, 26.11%
aleksandrvk [35]

The molecular formula :

C₆H₁₄O₃PF

<h3>Further explanation</h3>

Given

39.10% carbon, 7.67% hydrogen, 26.11%  oxygen, 16.82% phosphorus, and 10.30% fluorine.

Required

The molecular formula

Solution

mol ratio :

C = 39.1 : 12 = 3.258

H = 7.67 : 1 = 7.67

O = 26.11 : 16 = 1.632

P = 16.82 : 31 = 0.543

F = 10.3 : 19 = 0.542

Divide by 0.542

C = 6

H : 14

O = 3

P = 1

F = 1

The empirical formula :

C₆H₁₄O₃PF

(The empirical formula)n = the molecular formula

(C₆H₁₄O₃PF)=184.1

(6.12+14.1+3.16+31+19)n=184.1

(184)n=184.1

n = 1

3 0
3 years ago
How many moles are in 1.505x10^24 molecules of surcrose
algol [13]

Answer:

2.499 moles of sucrose

Explanation:

Divide by Avogadro's number

5 0
3 years ago
How are elements identified in terms of their atoms
bazaltina [42]
An element is defined as a substance made up of atoms with a specific number of protons.
4 0
3 years ago
How many moles of ammonia would be required to react exactly with 0.470 moles of cooper (ll) oxide in the following chemical rea
larisa [96]

Answer:

0.313 mole of NH3

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

2NH3(g) + 3CuO(s) → 3Cu(s) + N2(g) + 3H2O(g)

The number of mole of ammonia (NH3) required to react with 0.470 mole of copper(ll) oxide (CuO) can be obtained as follow:

From the balanced equation above,

2 moles of NH3 reacted with 3 moles of CuO.

Therefore, Xmol of NH3 will react with 0.470 mole of CuO i.e

Xmol of NH3 = (2 x 0.470) /3

Xmol of NH3 = 0.313 mole.

Therefore, 0.313 mole of NH3 is needed for the reaction

4 0
3 years ago
What is the solubility of ethylene (in units of grams per liter) in water at 25 °C, when the C2H4 gas over the solution has a pa
vredina [299]

<u>Answer:</u> The solubility of ethylene gas in water is 9.16\times 10^{-2}g/L

<u>Explanation:</u>

To calculate the molar solubility, we use the equation given by Henry's law, which is:

C_{C_2H_4}=K_H\times p_{C_2H_4}

where,

K_H = Henry's constant = 4.78\times 10^{-3}mol/L.atm

C_{C_2H_4} = molar solubility of ethylene gas = ?

p_{C_2H_4} = partial pressure of ethylene gas = 0.684 atm

Putting values in above equation, we get:

C_{C_2H_4}=4.78\times 10^{-3}mol/L.atm\times 0.684atm\\\\C_{C_2H_4}=3.27\times 10^{-3}mol/L

Converting this into grams per liter, by multiplying with the molar mass of ethylene:

Molar mass of ethylene gas = 28 g/mol

So, C_{C_2H_6}=3.27\times 10^{-3}mol/L\times 28g/mol=9.16\times 10^{-2}g/L

Hence, the solubility of ethylene gas in water is 9.16\times 10^{-2}g/L

6 0
3 years ago
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