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Vladimir79 [104]
4 years ago
9

Approximately how much greater in mass is a d2o molecule than an h2o molecule? (assume the oxygen atoms have a mass number of 16

. deuterium, d, is an isotope of hydrogen with a mass number of 2, 2h.)
Chemistry
2 answers:
faust18 [17]4 years ago
6 0

The deuteriuoted water that is D_{2}O consists of an isotope of hydrogen in place of hydrogen from the normal water. The approximate mass of deuteriuoted water and normal water can be calculated as {(2×2)+16} = 20. However the exact mass of D_{2}O is 20.027 g/mole, whereas the mass of water can also be calculated as- {(1×2)+16}=18, however the exact mass of (H_{2}O) molecule is 18.015 g/mole. Thus the difference between the mass of the molecules are (20.027 - 18.015) = 2.01 2g/mole.

7nadin3 [17]4 years ago
3 0

Answer:

D_2O molecule is greater than H_2O molecule by 2 amu.

Explanation:

Mass of H_2O molecule:

M_{H_2O}= 2 × 1 amu + 1 × 16 amu = 18 amu

Mass of D_2O molecule:

M_{D_2O}= 2 × 2 amu + 1 × 16 amu = 20 amu

Difference between mass of D_2O \& H_2O

M_{D_2O}-M_{H_2O} =20 amu - 18 amu = 2 amu

M_{D_2O} =2+M_{H_2O}

D_2O molecule is greater than H_2O molecule by 2 amu.

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Escaping from the haunted house, Anna ran home immediately to her chemistry lab
nevsk [136]
89.1% Au

The molar mass of Au2O3 is 2(196.97) + 3(16.00) = 441.94 g/mol
The mass percent of Au is therefore 2(196.97) / 441.94, which is 393.94/441.94 = 0.891 —> 89.1%
6 0
3 years ago
How many molecules are in 42.3g sample of water
Helga [31]

Answer:

The number of molecules is 1.4140*10^24 molecules

Explanation:

To know the number of molecules, we need to determine how many moles of water we have, water has molar mass of 18.015g/mol

This means that one mole of water molecules has a mass of 18.015g.

42.3g * 1 mole H2O/18.015g

= 2.3480 moles H2O

We are using avogadros number to find the number of molecules of water

2.3480 H2O * 6.022*10^ 23moles/ 1mole of H2O

That's 2.3480 multiplied by 6.022*10^23 divided by 1 mole of H2O

Number of molecules = 1.4140 *10^24 molecules

5 0
3 years ago
A container holds 35.8 moles of gas under 10.0 atm of pressure at 70.0 C. What is the volume of the container?
zhenek [66]
THE ANSWER

for solving this, we just use the formula of the equation of state

PV = n RT
where
P: pressure =10atm
V volume
n number of mole = 35.8 moles
R universal gas constant = 0.082
T: The temperature= 70°C= 343.15 Kelvin

therefore, for finding V
we have 
 
V= (n RT) / P = 35.8 x 0.082 x 343.15   / 10 = 100.7 ≈ 101 L

the answer is V = 101L






3 0
4 years ago
Which of the following processes will determine the number of moles in a sample? Dividing the mass of the sample by Avogadro's n
Olenka [21]

The answer is: Dividing the number of molecules in the sample by Avogadro's number.

The Avogadro’s number is the number of atoms in 12 grams of the isotope carbon-12 (¹²C).

Na is Avogadro number or Avogadro constant (the number of particles, in this example carbon, that are contained in the amount of substance given by one mole).

The Avogadro number has value 6.022·10²³ 1/mol in the International System of Units; Na = 6.022·10²³ 1/mol.

For example:

N(Ba) = 2.62·10²³; number of atoms of barium.

n(Ba) = N(Ba) ÷ Na.

n(Ba) = 1.3·10²⁴ ÷ 6.022·10²³ 1/mol.

n(Ba) = 2.158 mol; amount of substance of barium.

6 0
3 years ago
13 points for this, you have to show how you did it because i need to figuer out how you did it.
andrey2020 [161]
CO + 2 H2 → CH3OH 
<span> find # of mols in each reactants, </span>

<span>152500 g CO x 1 mol CO / 28.01g CO = 5444 mol CO </span>

<span>24500 g H2 x 1 mol H2 / 2.02 g H2 = 12129 mol H2 </span>

<span>mol ratio between CO and H2 is 1:2, which means each mol of production of CH3OH need 1 mol of CO and 2 mol of H. </span>

<span>H2 is enough to produce 6064 mols of CH3OH but there are only 5444mol of CO. </span>

<span>5444 mol CH3OH x molar mass of CH3OH / 1 mol CH3OH </span>

<span>= 174371 g = 174.4 kg</span>
4 0
3 years ago
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