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3 years ago

How many moles of ions are produced by the dissociation of 0.5 mol of na2co3?

2 answers:

tatiyna3 years ago

5 0

The number of moles of ions that are produced by the dissociation of o.5 mol of Na2CO3 is 1.5 moles

Explanation
write the equation for dissociation of Na2CO3
that is Na2Co3 → 2Na^+(aq) + CO3^2- (aq)

by use of mole ratio of Na2CO3 to Na^+ and to CO3^2- which is 1:2:1 the moles of Na^+ = 0.5 x2 = 1mole
the moles of CO3^2- = 0.5 x1 = 0.5 moles

total moles = moles of CO^2- + moles of Na^+

that is 1 mole + 0.5 mole = 1..5 moles

Alexus [3.1K]3 years ago

3 0

Answer:

1.5 mol ions

Explanation:

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olchik [2.2K]

Answer:

The correct options are:

B. The HCl is the solute.

D. The H₂O is the solvent.

E. This mixture conducts electricity.

Explanation:

For the preparation of the HCl solution, 10 mL of HCl and 40 mL of water were mixed.

The compound that is present in the solution in a smaller ratio is the solute and the other compount -present in higher ratio- is the solvent.

So, the solute is HCl and the solvent is water (H₂O). Furthermore, water is considered as an universal solvent (for most of the polar and ionic compounds). According to this, the following options are correct:

B. The HCl is the solute.

D. The H₂O is the solvent.

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3 years ago

A 16.0 g sample of methane gas, CH4, the gas used in a chemistry lab, has a volume of 5.0 L at 27ºC. Calculate the pressure.

NeX [460]

Answer:

4.9 atm

Explanation:

convert 16.0g of CH4 to moles

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2 years ago

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lianna [129]

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3 years ago

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3 years ago

1. If 3.25 moles of oxygen were consumed, how much moles of carbon dioxide are produced?

liraira [26]

Answer:

3.25 mol CO₂

Explanation:

Step 1: Write the balanced equation

C(s) + O₂(g) ⇒ CO₂(g)

Step 2: Establish the appropriate molar ratio

According to the balanced equation, the molar ratio of O₂ to CO₂ is 1:1.

Step 3: Calculate the number of moles of CO₂ produced from 3.25 moles of O₂

We will use the previously established molar ratio.

3.25 mol O₂ × 1 mol CO₂/ 1 mol O₂ = 3.25 mol CO₂

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