All categories

3 years ago

Q8. Which of these results when a neutral atom gains an electron? *

Chemistry

1 answer:

aliina [53]3 years ago

6 0

Answer:

Explanation:

it becomes a positive charge and fully filled

You might be interested in

Enter your answer in the provided box. Liquid methanol (CH3OH) can be used as an alternative fuel in pickup and SUV engines. An

andreyandreev [35.5K]

Answer: E=∆H*n= -40.6kj

Explanation:

V(CO) =15L=0.015M³

P=11200Pa

T=85C=358.15K

PV=nRT

n=(112000×0.015)/(8.314×358.15)

n(Co)= 0.564mol

V(Co)= 18.5L = 0.0185m³

P=744torr=98191.84Pa

T= 75C = 388.15k

PV=nRT

n= (99191.84×0.0185)/(8.314×348.15)

n(H2) = 0.634mol

n(CH30H) =1/2n(H2)=1/2×0.634mol

=0.317mol

∆H =∆Hf{CH3OH}-∆Hf(Co)

∆H=-238.6-(-110.5)

∆H = 128.1kj

E=∆H×n=-40.6kj.

3 0

3 years ago

Calculate the osmotic pressure of a 5.5M glucose solution at 20 degrees Celsius

NeTakaya

The osmotic pressure is a colligative property which depends upon the number of molecules and not the type of molecules

The relation between osmotic pressure and concentration is

πV = nRT

where

π = Osmotic pressure [ unit atm] = ?

V = volume

n = moles

R = gas constant = 0.0821 L atm / mol K

T = temperature = 20°C = 20 + 273.15 K = 293.15 K

also

Molarity = moles / Volume

Molarity = n/V = 5.5 M

Putting values

π = MRT

π = 5.5 X 0.0821 X 293.15 = 132.37 atm

Osmotic pressure of given glucose solution will be 132.37 atm

5 0

4 years ago

Write formulas and names for two binary molecular compounds

lyudmila [28]

Answer:

NaCl sodium chloride

HF hydrogen flouride

Explanation:

7 0

3 years ago

What is an example of a chemical bond

KatRina [158]

Sodium Chloride or NaCl is a ionic bond

3 0

3 years ago

How much volume will 8.8 moles of gas fill at 0.12 atm at 56*C

Neporo4naja [7]

Answer:

2000 L

General Formulas and Concepts:

Atomic Structure

Moles
Temperature Conversion: K = °C + 273.15

Gas Laws

Ideal Gas Law: PV = nRT

P is pressure
V is volume (in L)
n is number of moles
R is gas constant
T is temperature (in K)

Explanation:

Step 1: Define

[Given] 8.8 moles gas

[Given] 0.12 atm

[Given] 56 °C = 329.15 K

Step 2: Solve for V

Substitute in variables [Ideal Gas Law Formula]: $\displaystyle (0.12 \ atm)V = (8.8 \ mol)(0.0821 \ \frac{L \cdot atm}{mol \cdot K})(329.15 \ K)$
Isolate V: $\displaystyle V = \frac{(8.8 \ mol)(0.0821 \ \frac{L \cdot atm}{mol \cdot K})(329.15 \ K)}{(0.12 \ atm)}$
Multiply/Divide [Cancel out units]: $\displaystyle V = 1981.7 \ L$

Step 3: Check

Follow sig fig rules and round. We are given 2 sig figs.

1981.7 L ≈ 2000 L

3 0

3 years ago