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tensa zangetsu [6.8K]
3 years ago
8

Question 6 of 10

Chemistry
1 answer:
KengaRu [80]3 years ago
8 0

Answer:

option C

Explanation:

hope it helps u

.......

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An ideal gas has a density of 1.10×10−6 g/cm3 at 1.00×10−3 atm and 80.0 ∘c. identify the gas.
True [87]
From  ideal  gas  equation  that  is pv =nRt
n=
number  of  moles which  can  be  written  as  the  ratio  between the  weight  of  a gas that  is mass and  its  molecular  mass  n=m/Mm
pv=(m/Mm)RT
density  is=mass  per  unit volume
P=m/v by  arranging  the  equation  we  get
R =0.082atm/mol/k
Mm=pRT/P=[(1.10  x10^-6 x1000g/l) xo.082  atm/mol/k x(80+273] /(1.00  x10^-3) =31.84  to the  nearest ten is  32
hence  the  gas  is  oxygen 
7 0
3 years ago
Please help! I’m on my last attempt
deff fn [24]
First line: The atomic number is the whole number on the periodic table so atomic number 35 means the element is bromine. Thus the element symbol is Br. The atomic number is also the number of protons in the isotope so the number of protons is 35. The mass number is the sum of protons and neutrons in the isotope so the mass number is 35+46 or 81. The mass number gives you the top left number on the nuclear symbol (it will look the same as the one below it except the 79 is an 81). Lastly, the number of electrons is equal to the number of protons in a neutral atom so 35 electrons.
6 0
3 years ago
when a reactive metal is added to water, bubbles or fizzing can be observed. Explain the appearance of the bubbles​
MakcuM [25]

Answer:

This is because of the release of hydrogen gas in the reaction.

Explanation:

Metals react with water and produce a metal oxide and hydrogen gas. It also starts floating due to the bubbles of hydrogen gas sticking to its surface.

For eg:

<u>2Mg. + 2H2O --------> 2MgOH + H2</u>

Here,

Metal taken is <u>magnesium(2Mg)</u> which when reacts with <u>water(2H2O)</u> to form its <u>oxide form (2MgOH)</u> and <u>hydrogen gas(H2)</u> is released which comes outside water as bubbles.

7 0
2 years ago
By process of incineration, a mystery substance is empirically determined to contain 40.00% carbon by weight, 6.67% hydrogen, an
Keith_Richards [23]

Answer:

C₂H₄O₂

Explanation:

Step 1: Divide each percentage by the atomic mass of the element

C: 40.00/12.01 = 3.331

H: 6.67/1.01 = 6.60

O: 53.33/16.00 = 3.333

Step 2: Divide all the numbers by the smallest one

C: 3.331/3.331 = 1

H: 6.60/3.331 ≈ 2

O: 3.333/3.331 ≈ 1

The empirical formula is CH₂O, with a molecular weight of 12 g/mol + 2 × 1 g/mol + 16 g/mol = 30 g/mol. The molecular weight of the compound must be a product of 30, such as 60 (between 55 and 62 g/mol). Since we have to multiply by 2 (30 to 60) to get to the molecular weight of the compound, we also have to multiply the empirical formula by 2 to get the chemical formula of the compound.

CH₂O × 2 = C₂H₄O₂

4 0
2 years ago
If an object loses mass, what will happen to its weight?
Sophie [7]
The answer is B. The less mass then the less the gravity pulls on it
8 0
3 years ago
Read 2 more answers
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