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3 years ago

Can someone help me with this question ASAP

Chemistry

1 answer:

Mkey [24]3 years ago

6 0

Aye i can’t see the full question dawg, you gotta send a full picture of it

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6. What is the molecular formula for this compound? The compound's empirical formula and

igomit [66]

Explanation:

A compound's empirical formula tells you the smallest whole number ratio ,The molar mass tells you what the total mass of one mole

6 0

3 years ago

Please help me with this question<br> Thank you!

Elza [17]

Answer:

B. 3+

Explanation:

When Fe²⁺ loses an electron, it becomes an Fe³⁺ ion.

The loss of an electron in an atom makes the atom becomes positively charged. Further losing electrons makes the atom more positive.

For the given ion;

Fe²⁺ if it loses an electron more, it becomes Fe³⁺.

The expression is given as:

Fe²⁺ → Fe³⁺ + e⁻

8 0

3 years ago

I Really Need Help:(

GarryVolchara [31]

Semi-conductor,brittle not malleable or ductile.

3 0

4 years ago

How many mL of .1250 M KCl solution contains 2.330g of KCl? KCl = 74.55 amu

lozanna [386]

The amu is a unit which means the mass per neutron, So the 74.55 means the mass per mole KCl. So the mole number of 2.330g KCl is 2.330/74.55=0.031 mol. The volume is 0.031/0.1250=0.248 L ≈ 250 mL. So the answer is a.

8 0

3 years ago

A mixture of hydrocarbons contains 38.3% hexane, C6H14, 13.9% octane, C8H18, and 47.8% decane, C10H22. The mixture is combusted

GaryK [48]

Answer:

52.206 kg

Explanation:

From the given information:

Mass of hexane C6H14 = $19.3*10^3 \ g \times \dfrac{38.3}{100}$

= 7391.9 g

Mass of octane C8H18 = $19.3*10^3 \ g \times \dfrac{13.9}{100}$

= 2682.7 g

Mass of decane C10H22 = $19.3*10^3 \ g \times \dfrac{47.8}{100}$

= 9225.4 g

However, recall that:

number of moles of an atom = mass/molar mass

∴

For hexane, no of moles = 7391.9 g/86.18 g/mol

= 85.77 moles

For octane, no of moles = 2682.7 g/114.23 g/mol

= 23.49 moles

For decane, no of moles = 9225.4 g/142.29 g/mol

= 64.84 moles

Therefore:

number of moles of CO2 produced = (6 × 85.77)+(23.49)+(10×64.84) moles

= 1186.51 moles

Finally, the mass of CO2 produced is:

= 1186.51 mol × 44 g/mol

= 52206.44 g

= 52.206 kg

4 0

3 years ago