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3 years ago

(a) How much negative charge is on each oxygen of the carbonate ion?

1 answer:

6 0

The chemical formula of a carbonate ion is CO3^2-. It is an AX3 system which means it take the trigonal planar shape. There would be two single bonds of C-O and one double bond C-O in order for C to agree with the octet rule. Two minus charges are equally distributed to the three oxygen atoms so that each oxygen of the carbonate ion would have a charge of negative 2/3.

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Balance the following equations: (c) H2(g)+I2(s)⟶HI(s)H2(g)+I2(s)⟶HI(s)

kenny6666 [7]

Answer: $H_2(g)+I_2(g)\rightarrow 2HI(s)$

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

Thus in the reactants, there are 2 atoms of hydrogen and 2 atoms of iodine .Thus there has to be 2 atoms of hydrogen and 2 atoms of iodine in the product as well. Thus a coefficient of 2 is placed in front of HI.

The balanced chemical reaction is:

$H_2(g)+I_2(g)\rightarrow 2HI(s)$

6 0

4 years ago

How much heat is produced by combustion 125 g of methanol under standard state condaitions?

timurjin [86]

Answer:

Explanation:

For the reaction ,

2CH₃OH + 3O₂ → 2CO₂ + 4 H₂O

For the above reaction ,

the change in enthalphy is calculated as

Δ Hrxn = Δ H°f (products) - Δ H°f (reactants)

In case the compound is in its standard state , enthalphy of formation is zero

Hence ,

for the above reaction ,

ΔHrxn =( 2 * Δ H° (CO₂ ) + 4 * Δ H° (H₂O )) - [ ( 2 *Δ H°CH₃OH ) + (3 * Δ H° O₂ )]

Δ H° (CO₂ ) = -393.5kJ /mol

Δ H° (H₂O ) = - 241.8 kJ /mol

Δ H°CH₃OH = -239.2kJ /mol

Δ H° O₂ = 0

putting the corresponding values ,

ΔHrxn =( 2 * -393.5kJ /mol + 4 *- 241.8kJ /mol) - [ ( 2 *-239.2kJ /mol ) + (3 *0 )

ΔHrxn = -1275.8 kJ /mol

Moles of methanol,

Moles is denoted by given mass divided by the molecular mass ,

Hence ,

n = w / m

n = moles ,

w = given mass ,

m = molecular mass .

From the question ,

w = 125 g

as we know ,

m = 32 g /mol

n = 125 g / 32 g /mol = 3.906 mol

From , the reaction , 2 mol produces -1275.8 kJ /mol heat ,

Now using unitary method ,

1 mol produces = -1275.8 kJ /mol / 2 heat ,

3.906 mol produces = -1275.8 kJ /mol / 2 * 3.906 heat

3.906 mol produces = 249.7 kJ

5 0

3 years ago

An alkali metal with fewer than 10 protons in its nucleus answer

otez555 [7]

The answer is beryllium

5 0

4 years ago

Read 2 more answers

Upon balancing the equation below, how many moles of calcium chloride are needed to react completely with 4.3 moles of silver ni

Lapatulllka [165]

2.2 mol CaCl<span>2 is the answer. </span>

7 0

3 years ago

Read 2 more answers

An element X has two naturally occurring isotopes: X-35 (abundance = 75.77%, mass = 34.968852 amu) and X-37 (abundance = 24.23%,

ipn [44]

Answer:

x = 35.453 amu. CHLORINE

Explanation:

Abundance of X³⁵ = 75.77%

Abundance of X³⁷ = 24.23%

Atomic mass of X³⁵ = 34.968852 amu

Atomic mass of X³⁷ = 36.965903 amu

Average atomic mass = ?

Solution:

Average atomic mass of carbon = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass) / 100

Average atomic mass of carbon = (34.968852 × 75.77)+(36.965903 ×24.23) /100

Average atomic mass of carbon= 2649.59 + 895.684 / 100

Average atomic mass of carbon = 3545.274 / 100

Average atomic mass of carbon = 35.453 amu.

x = 35.453 amu. CHLORINE

5 0

4 years ago