Which functional group is within the compound shown below?

Molten gallium reacts with arsenic to form the semiconductor, gallium arsenide, GaAs, used in light-emitting diodes and solar ce

Vsevolod [243]

Answer:

a) 1.2g of arsenic b) 0.64g of arsenic c) 3.481g of gallium d) 3.806g of gallium e) 2.61g arsenic

Explanation:

The balanced equation is:

Ga + As = GaAs, 1:1 mole ratio

a) mass (gallium)/ molar mass of Ga = 4/ 69.723 = 0.0574mol

Mass (arsenic)/ molar mass of As = 5.5/74.9216 = 0.0734, subtracting the moles from each other (knowing already that the ratio is 1:1), arsenic is in excess by 1.2g

b) repeating the procedure (changing the values)

It will be 0.0574 to 0.06593

Arsenic is in excess by 0.00854

0.00854* mass of arsenic (such must be done for the first remaining mole) = 0.64g

c) the mole ratio is 0.0574: 0.00747

Gallium is in excess by 0.05

Mass of excess gallium = 0.05* 69.723 = 3.481g

d) using the mass given, the new ratio is

0.128: 0.0734

Gallium is in excess by 0.054mol

Mass of excess gallium = 0.054*69.723 = 3.806g

e) using the mass again, the new ratio is 0.0574: 0.02,

Gallium is in excess by 0.0374*69.723 = 2.61g

7 0

4 years ago

while looking at neon on the periodic table a student needs to find an element with a smaller atomic mass in the same group wher

Oxana [17]

In the noble gasses section. Above neon is helium, which means it has less atomic mass, and is in the same section

7 0

3 years ago

Read 2 more answers

If a long steady rain is expected which clouds should be expected

Inessa [10]

Nimbostratus clouds bring long steady rains

4 0

4 years ago

How many molecules of ethane ( C2H6) are present in 0.197g of C2H6?

Brut [27]

Answer:

3.945 x 10²¹ molecules

Explanation:

Firstly, we need to calculate the no. of moles using the relation:

n = mass/molar mass = (0.197 g)/(30.07 g/mol) = 6.55 x 10⁻³ mol.

It is known that every 1.0 mol of a molecule contains Avogadro's number of molecules (NA = 6.022 x 10²³).

<em>∴ 0.197 g of C₂H₆ will contain</em> = (6.55 x 10⁻³ mol)(6.022 x 10²³) = <em>3.945 x 10²¹ molecules.</em>

4 0

3 years ago

Read 2 more answers

Liquid octane (CH) has a density of 0.7025 g/mL at 20 °C. Find the true mass (murue) of octane when the mass weighed in 18 air i

Goshia [24]

Explanation:

According to Buoyance equation,

m = $[m' \times \frac{1 - \frac{d_{a}}{d_{w}}}{1 - \frac{d_{a}}{d}}]$

where, m = true mass

m' = mass read from the balance = 17.320 g

$d_{a}$ = density of air = 0.0012 g/ml

$d_{w}$ = density of the balance = 7.5 g/ml

d = density of liquid octane = 0.7025 g/ml

Now, putting all the given values into the above formula and calculate the true mass as follows.

m = $[m' \times \frac{1 - \frac{d_{a}}{d_{w}}}{1 - \frac{d_{a}}{d}}]$

= $[17.320 g \times \frac{1 - \frac{0.0012 g/ml}{7.5 g/ml}}{1 - \frac{0.0012 g/ml}{0.7025}}]$

= $17.320 g \times 0.999850$

= 17.317 g

Thus, we can conclude that the true mass of octane is 17.317 g.

7 0

3 years ago