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2 years ago

What is the length of the shaded grey area? write your answer to the correct number of significant digits. The unit is cm

Chemistry

1 answer:

alukav5142 [94]2 years ago

8 0

Answer:

1.37cm

Explanation:

It's less than 1.4cm but more than 1.3cm. It's also more than 1.35cm so I guess the best answer would be 1.37cm or round up to 1.4cm

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2, 3-diethyl–4-octene what is structure of this pls help

pantera1 [17]

Answer:

(CH2CH3).

CH-CH-CH-CH=CH-CH2-CH2-CH3

(CH2CH3)

2, 3-diethyl–4-octene

i am not sure.

4 0

3 years ago

A student makes a sandwich with several layers of bread and cheese. Then the student cuts the sandwich and says it models how a

Ksenya-84 [330]

Answer:

Rock layer and sandwich layer is almost the same.

Why are rock layers are like sandwiches?

This geologic structure is called an anticline. Now gently bend your sandwich so that the layers are bowed downwards, thus creating a syncline. The presence of anticlines and synclines indicate strong forces that often form mountain ranges.

7 0

3 years ago

Choose the element described by the following electron configuration. 1s22s22p63s23p64s1

Jobisdone [24]

Hey there.

By adding up all the "exponents," you'll get a number of 19. By looking at a periodic table, the element of such an atomic number is potassium or K.

3 0

4 years ago

Read 2 more answers

A mixture of helium, nitrogen, and oxygen has a total pressure of 752 mm Hg. The

NISA [10]

Answer: The partial pressure of oxygen in the mixture is 321 mm Hg

Explanation:

According to Dalton's law, the total pressure is the sum of individual pressures.

$p_{total}=p_{He}+p_{N_2}+p_{O_2}$

Given : $p_{total}$ = total pressure of gases = 752 mm Hg

$p_{He}$ = partial pressure of Helium = 234 mm Hg

$p_{N_2}$ = partial pressure of nitrogen = 197 mm Hg

$p_{O_2}$ = partial pressure of oxygen = ?

Putting in the values we get:

$752mmHg=234mmHg+197mmHg+p_{O_2}$

$p_{O_2}=321mmHg$

The partial pressure of oxygen in the mixture is 321 mm Hg

5 0

3 years ago

1. Compare masses: a) 0,4mol CO₂ and 0,6mol H₂O ; b) 0,135mol H₂SO₄ and 0,5mol HCI.

bixtya [17]

Answer:

you can now deduct which one is greater or smaller and by how much.

Explanation:

no of moles= mass/molar mass

1ai) 0.4 = m/ ( 12 + (16*2)

m= 0.4* 44

m= 17.6g

ii) 0.6= m/( 2*1 + 16)

m= 0.6 *18

m= 10.8g

b) 0.135 = m/ ( 2*1 +32 + (16*4)

m= 0.135* 98

m= 13.23g

ii) 0.5= m/ (1+35.5)

m= 0.5*36.5

m= 18.25g

2. Avogadro's Number = 6.02×10²³

1 mol of any element= 6.02×10²³ particles

a) 0.1 mol of H20= (6.02×10²³) * 0.1

= 6.02×10²² molecules

ii) 0.3 mol of CO2= (6.02×10²³) * 0.3

= 1.806 × 10²³ molecules

Ans: 0.3 mol of CO2

bi) 0.25 mol of HCl= (6.02×10²³) * 0.25

= 1.505 × 10²³ molecules

bii) - find the no of moles first:

no of moles= mass/molar mass

n= 3.4g/ 34g →mr of H2S in g=2+32= 34g

n= 0.l mol

- use the Avogadro Number.

0.1 mol of H20= (6.02×10²³) * 0.1

= 6.02×10²² molecules.

biii) here you're given the density, use it to find the mass of acetic acid.

ρ = 1049 g/ml

ρ = m/v, where v=5 ml

1049 = m/ 5

m= ρ*v

m= 1049*5

m= 5245 g

• convert this into moles.

mr of CH3COOH= 12 + 3+ 12+ 16+ 16+ 1

= 60

mr in g = 60g

n= m/mr

n= 5245/ 60

n= 87. 41666...

n= 87.4 moles

•using Avogadro's Number:

87.4 moles of acetic acid=(6.02×10²³)*87.4

= 2.25148* 10²⁵

= 2.25 * 10²⁵ molecules

thus, the ans for this is 5 ml of acetic acid.

7 0

2 years ago