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JulsSmile [24]
3 years ago
5

Ion If we add an electron to a stable element we call it a(n)_____ion anion cation

Chemistry
1 answer:
masha68 [24]3 years ago
3 0
The answer is a cation, I may be wrong but cation is plus and anion is subtract
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Give the ion symbol for the the ion that has 15 protons and 18 electrons
Montano1993 [528]
By referring to a periodic table or table of elements, we see that phosphorus (symbol P) has an atomic number of 15. Thus, each atom has 15 protons. The mass number of the ion is 15 + 16 = 31. Because the ion has 15 protons and 18 electrons (three more electrons than protons), its net charge is 3-.
7 0
3 years ago
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An unidentified compound contains only phosphorous and fluorine, meaning we could write its formula as PxFy. Heating 0.2324 g of
cricket20 [7]

Answer:

The molecular formula of the compound is P2F4

Explanation:

Step 1: Data given

Mass of the compound  = 0.2324 grams

Volume of container = 378 mL

Pressure at 77 °C = 97.3 torr

The gaseous PxFy was then reacted with an aqueous solution of calcium chloride, and all of the fluorine was converted to 0.2631 g of CaF2.

Molar mass CaF2 = 78.07 g/mol

Step 2: Calculate moles CaF2

Moles CaF2 = 0.2631 g/ 78.07 g/mol=0.003370

Step 3: Calculate moles F

For every 1 mol CaF2 we have 1 mol Ca2+ and 2 moles F-

moles F- = 2 * 0.003370=0.006740

Step 4: Calculate mass of F

mass F =  0.006740 mol * 19.00 g/mol=0.1281 g

Step 5: Calculate mass of P

mass P = mass of compound - mass of F = 0.2324 - 0.1281 =0.1043 g

Step 6: Calculate moles P

moles P = 0.1043 g/ 30.97 g/mol=0.003368 moles

Step 7: Calculate mol ratio

We divide by the smallest amount of moles

P: 0.003368/0.003368 =1

F: 0.006740/ 0.003368 =2

The empirical formula is PF2

The empirical formula has a molar mass of 68.97 g/mol

Step 8: Calculate moles of compound

p*V = n*R*T

n = (p*V)/(R*T)

⇒ with p = the pressure of the gas = 97.3 torr = 97.3/760 = 0.128 atm

⇒ with V = the volume of the gas = 0.378 L

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T = the temperature = 77.0 °C = 350 Kelvin

Number of moles =(0.128 *0.378)/(0.08206*350)

Number of moles =

moles gas = pV/RT = 0.128 atm x 0.378 dm^3/ 0.08206x350 K=0.00168  

Step 9: Calculate molar mass

Molar mass = mass / moles

Molar mass = 0.2324 grams / 0.00168 moles

Molar mass = 138 g/mol

Step 10: Calculate the molecular formula

138.0 / 68.97 = 2

2*(PF2) = P2F4

The molecular formula of the compound is P2F4

4 0
3 years ago
Calculate the amount of heat necessary to raise the temperature of 135.0 g of water from 50.4°F to 85.0°F. The specific heat of
MAXImum [283]

Here we have to calculate the heat required to raise the temperature of water from 85.0 ⁰F to 50.4 ⁰F.

10.857 kJ heat will be needed to raise the temperature from 50.4 ⁰F to 85.0 ⁰F

The amount of heat required to raise the temperature can be obtained from the equation H = m×s×(t₂-t₁).

Where H = Heat, s  =specific gravity = 4.184 J/g.⁰C, m = mass = 135.0 g, t₁ (initial temperature) = 50.4 ⁰F or 10.222 ⁰C and t₂ (final temperature) = 85.0⁰F or 29.444 ⁰C.

On plugging the values we get:

H = 135.0 g × 4.184 J/g.⁰C×(29.444 - 10.222) ⁰C

Or, H = 10857.354 J or 10.857 kJ.

Thus 10857.354 J or 10.857 kJ heat will be needed to raise the temperature.

6 0
3 years ago
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kenny6666 [7]

Answer:

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Explanation:

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Consider the reaction pathway graph below.
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E and Dis determine the H
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