What is the mass of 4.57 x 1021 molecules of ammonia (NH3)?

How many moles of iron (Fe) will be produced from 6.20 moles of carbon monoxide (CO)

anzhelika [568]

Answer:

4.13 moles of Fe will be produced in the reaction

Explanation:

To produce Fe from CO, we need to react Fe₂O₃ and the carbon monoxide.

The reaction is:

Fe₂O₃ + 3CO → 2Fe + 3CO₂

1 mol of iron (III) oxide react to 3 moles of carbon monoxide in order to produce 2 moles of Iron and 3 moles of carbon dioxide.

We assume, the Fe₂O₃ in excess, so we propose this rule of three

3 moles of CO can produce 2 moles of Fe

Therefore 6.20 moles of CO will produce (6.20 . 2)/3 = 4.13 moles of Fe

4 0

3 years ago

Read 2 more answers

What is a covalent bond

diamong [38]

Answer:

Covalent bonds involve the sharing of electron pairs between atoms. Electron pairs shared between atoms of equal or very similar electronegativity constitute a nonpolar covalent bond (e.g., H–H or C–H), while electrons shared between atoms of unequal electronegativity constitute a polar covalent bond (e.g., H–O).

Explanation:

8 0

3 years ago

Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or

Ahat [919]

Answer :

Oxidation number or oxidation state : It represent the number of electrons lost or gained by the atoms of an element in a compound.

Oxidation numbers are generally written with the sign (+) and (-) first and then the magnitude.

Rules for Oxidation Numbers are :

The oxidation number of a free element is always zero.
The oxidation number of a monatomic ion equals the charge of the ion.
The oxidation number of Hydrogen (H) is +1, but it is -1 in when combined with less electronegative elements.
The oxidation number of oxygen (O) in compounds is usually -2.
The oxidation number of a Group 17 element in a binary compound is -1.
The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.
The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

Now we have to determine the oxidation state of the elements in the compound.

(a) $H_2SO_4$

Let the oxidation state of 'S' be, 'x'

$2(+1)+x+4(-2)=0\\\\x=+6$

Hence, the oxidation state of 'S' is, (+6)

(b) $Ca(OH)_2$

Let the oxidation state of 'Ca' be, 'x'

$x+2(-2+1)=0\\\\x=+2$

Hence, the oxidation state of 'Ca' is, (+2)

(c) $BrOH$

Let the oxidation state of 'Br' be, 'x'

$x+(-2)+1=0\\\\x=+1$

Hence, the oxidation state of 'Br' is, (+1)

(d) $ClNO_2$

Let the oxidation state of 'N' be, 'x'

$-1+x+2(-2)=0\\\\x=+5$

Hence, the oxidation state of 'N' is, (+5)

(e) $TiCl_4$

Let the oxidation state of 'Ti' be, 'x'

$x+4(-1)=0\\\\x=+4$

Hence, the oxidation state of 'Ti' is, (+4)

(f) $NaH$

Let the oxidation state of 'Na' be, 'x'

$x+(-1)=0\\\\x=+1$

Hence, the oxidation state of 'Na' is, (+1)

4 0

3 years ago

What is the charge of GaF3

slavikrds [6]

Answer:

This charge transfer led to the formation of pentacoordinated square pyramidal MX·(YZ3) adducts with M·Y dative bond. Binding energies were -44.7 and -75.2 kcal/mol for interaction of GaF3 as the strongest acid with PtNCN

4 0

3 years ago

How many grams of dry NH4Cl need to be added to 2.10L of a 0.700M solution of ammonia, NH3, to prepare a buffer solution that ha

dezoksy [38]

I got 9.25527 for the pKa
then for the Henderson-Hasselbalch equation: 
9.00=9.25527+log(.600/acid) 
10^(-.25527)=(.600/acid)correct to this line. Then
0.5556 = 0.6/acid and
acid = 0.6/0.5556 = 1.08 which is the reciprocal of your number)

.5556/.600M=acid 
acid=.925925...M 
(.925925)*2.10L= Molarity

4 0

3 years ago