All categories

3 years ago

Can someone please help by filling out this table?

Chemistry

1 answer:

tamaranim1 [39]3 years ago

5 0

Answer:

Lithium looses one electron.

The charge - $Li^{+}$ - Cation

Nitrogen gains three electrons - $Ni^{3-}$ - Anion

Boron losses three electron.

The charge - $B^{3+}$ - Cation

Explanation:

Lithium looses one electron.

The charge - $Li^{+}$ - Cation

Nitrogen gains three electrons - $Ni^{3-}$ - Anion

Boron losses three electron.

The charge - $B^{3+}$ - Cation

The complete table is as follows.

You might be interested in

Given the values of ΔGfo given below in kJ/mol, calculate the value of ΔGo in kJ for the combustion of 1 mole of butane to form

xz_007 [3.2K]

Answer:

Δ $_rG=-2753kJ$

Explanation:

Hello,

Butane's combustion is:

$C_4H_{10}+\frac{13}{2} O_2-->4CO_2+5H_2O$

Now the change in the Gibbs free energy for this reaction is computed via (don't forget that oxygen's Gibbs free energy of formation is 0 since it is an element):

Δ $_rG=$ 4Δ $_fG_{CO_2}+$ 5Δ $_fG_{H_2O}$ -Δ $_fG_{C_4H_{10}}$

Δ $_rG=4(-395kJ/mol)+5(-238kJ/mol)-(-17kJ/mol)$

Δ $_rG=-2753kJ/mol$

Now, since the calculation is done for 1 mol of butane, the change in the Gibbs free energy for this fuel is:

Δ $_rG=-2753kJ$

Best regards.

4 0

3 years ago

Formula for sodium iodine

Vlad1618 [11]

Nal is the formula for sodium iodine

6 0

3 years ago

Read 2 more answers

PLEASE HELP ME !!!!!!!

love history [14]

Answer:

it would be 5,045

Explanation:

because it is closer to 5,000. pls correct me if wrong

5 0

2 years ago

Which of the following statements is true regarding both theories and laws?

Mariana [72]

Answer:

D. Supported by observations

Explanation:

Because theories change over time, they both need to be proven, they do not go off of consensus, but they do need to be supported by observations.

HOPE IT HELPS❣️

6 0

2 years ago

How much heat is released when 24.8 g of ch4 is burned in excess oxygen gas?

balu736 [363]

The given question is incomplete. The complete question is:

How much heat is produced when 24.8 g of $CH_4$ is burned in excess oxygen gas

Given: $CH _4
+2O_2\rightarrow CO_2+2H_2O$ ΔH= −802 kJ.

Answer: 1243.1 kJ

Explanation:

Heat of combustion is the amount of heat released on complete combustion of 1 mole of substance.

Given :

Amount of heat released on combustion of 1 mole of methane = 802 kJ kJ/mol

According to avogadro's law, 1 mole of every substance occupies 22.4 L at NTP, weighs equal to the molecular mass and contains avogadro's number $6.023\times 10^{23}$ of particles.

1 mole of $CH_4$ weighs = 16 g

Thus we can say:

16 g of $CH_4$ on combustion releases heat = 802 kJ

Thus 24.8 g of $CH_4$ on combustion releases = $\frac{802}{16}\times 24.8=1243.1kJ$

Thus heat released when 24.8 g of methane is burned in excess oxygen gas is 1243.1 kJ

4 0

3 years ago