Helium is listed as a noble gas true or false

Which type of bonding forms due to electrical attractions between oppositely charged elements

deff fn [24]

Answer:

Explanation:

Ionic bond

Ionic bond, also called electrovalent bond, type of linkage formed from the electrostatic attraction between oppositely charged ions in a chemical compound.

5 0

4 years ago

100.0 g H2SO4 =<br> ? mole H2SO4

diamong [38]

Answer:

sulfuric acid ..............

6 0

3 years ago

A solid that forms and separates from a liquid mixture is a.......

inna [77]

A solid that forms and separates from a liquid mixture is a chemical change.

4 0

4 years ago

A reaction produced 37.5 L of oxygen gas at 307 K and 1.25 atm. How many moles of oxygen were produced? 0.538 mol, O2 1.86 mol,

zlopas [31]

Answer:

O 2 has a mass of 1.78g

Explanation:

We are at STP and that means we have to use the ideal gas law equation!

P represents pressure (could have units of atm, depending on the units of the universal gas constant)

V represents volume (must have units of liters)

n represents the number of moles

R is the universal gas constant (has units of

L

× a t m

m o l

×

K

)

T represents the temperature, which must be in Kelvins.

Next, list your known and unknown variables. Our only unknown is the number of moles of

O

2

(

g

)

. Our known variables are P,V,R, and T.

At STP, the temperature is 273K and the pressure is 1 atm. The proportionality constant, R, is equal to 0.0821

L

×

a

t

m

o

l

×

K

Now we have to rearrange the equation to solve for n

n

=

P

V

R

T

n

=

1

atm

×

1.25

L

0.0821

Lxxatm

m

o

l

×

K

×

273

K

n

=

0.05577

m

o

l

To get the mass of

O

2

, we just have to use the molar mass of oxygen as a conversion factor:

0.0577

mol

O

2

×

32.00

g

1

mol

= 1.78g

O

2

3 0

3 years ago

Read 2 more answers

etermine the molar concentration of magnesium ions in a solution formed by mixing 100.0 mL of 0.100 M MgCl, solution with 100.0

marysya [2.9K]

Answer:

Molar concentration of magnesium ions in the final solution is 0.2 M.

Explanation:

$c=\frac{n}{V}$

c = Concentration of the solution

n = moles of the compound

V = volume of the solution in L

1) Molarity of $MgCl_2$ solution = 0.100 M

Volume of $MgCl_2$ solution = 100.0 mL = 0.1 L

Moles of $MgCl_2$ in 100 mL solution= n

$0.100 M=\frac{n}{0.1L}$

$n=0.01 mol$

$MgCl_2(aq)\rightarrow Mg^{2+}(aq)+2Cl^-(aq)$

1 mole of magnesium chloride gives 1 mol of magnesium ions and 2 moles of chloride ions.

Then 0.01 moles of magnesium chloride will give:

$x=\frac{1}{1}\times 0.01 mol=0.01 mol$ magnesium ions.

2) Molarity of $Mg_3(PO_4)_2$ solution = 0.100 M

Volume of $Mg_3(PO_4)_2$ solution = 100.0 mL = 0.1 L

Moles of $Mg_3(PO_4)_2$ in 100 mL solution= n'

$0.100 M=\frac{n'}{0.1L}$

$n'=0.01 mol$

$Mg_3(PO_4)_2(aq)\rightarrow 3Mg^{2+}(aq)+2PO_{4}^-(aq)$

1 mole of magnesium phosphate gives 3 mol of magnesium ions and 2 moles of phosphate ions.

Then 0.01 moles of magnesium phosphate will give:

$y=\frac{3}{1}\times 0.01 mol=0.03 mol$ magnesium ions.

After mixing both solutions:

Moles of magnesium ions = x + y = 0.01 mol + 0.03 mol = 0.04 mol

Total volume after mixing = 0.1 L + 0.1 L = 0.2 L

Molar concentration of magnesium ions in the final solution: $[Mg^{2+}]$

$[Mg^{2+}]=\frac{0.04 mol}{0.2 L}=0.2 mol/L$

4 0

4 years ago