Balance equation of gas burns carbon dioxide and water

When an atom is unstable, what will happen?

nevsk [136]

Answer: Unstable atoms will lose neutrons and protons as they attempt to become stable, atoms the binding energy is not strong enough to hold the nucleus together

Explanation:

4 0

3 years ago

A mysterious white powder could be powdered sugar (C12H22O11), cocaine (C17H21NO4), codeine (C18H21NO3), norfenefrine (C8H11NO2)

konstantin123 [22]

Answer: norfenefrine $(C_8H_{11}NO_2)$

Explanation:

Depression in freezing point is given by:

$\Delta T_f=i\times K_f\times m$

$\Delta T_f=T_f^0-T_f=(-114.6-(-115.5)^0C=0.9^0C$ = Depression in freezing point

i= vant hoff factor = 1 (for non electrolyte)

$K_f$ = freezing point constant = $1.99^0C/m$

m= molality

$\Delta T_f=i\times K_f\times \frac{\text{mass of solute}}{\text{molar mass of solute}}\times \text{weight of solvent in kg}}$

Weight of solvent (ethanol)= $density\times volume=0.789g/cm^3\times 1.50cm^3=1.18g=1.18\times 10^{-3}kg$

Molar mass of unknown non electrolyte = M g/mol

Mass of unknown non electrolyte added = 82 mg = 0.082 g (1g=1000mg)

$0.9=1\times 1.99\times \frac{0.082g}{M g/mol\times 1.18\times 10^{-3}}kg}$

$M=154g/mol$

The molecular mass of norfenefrine $(C_8H_{11}NO_2)$ is near to 154 and thus the identity of the white powder is norfenefrine .

4 0

3 years ago

Write the expression for the equilibrium constant for this reaction. 2N205(g) <==> 4N02(g) + 02(g)

Elis [28]

Answer:

K = [NO₂]⁴[O₂] / [N₂O₅]²

Explanation:

Based on the chemical equilibrium reaction:

2 N₂O₅(g) ⇄ 4NO₂(g) + O₂(g)

The equilibrium reaction is obtained as the ratio between the multiplication of the concentrations of the reactants over the products powered to its reaction coefficient. That is:

7 0

3 years ago

I’ve been stuck on these 5 questions!? Can you guys help?!

Varvara68 [4.7K]

Answer:

1. 0.224 moles of oxygen

3. 143.36 L oxygen gas

5. 0.059 atm

10. 5.14 atm

11. 307 K

Explanation:

1. You have to use the ideal gas law: PV=nRT where P is pressure in atm, V is volume in liters, n is number of moles, R is the constant 0.08206 L atm mol^-1 K^-1, and T is the temperature in Kelvins where K=degrees celsius+273.15 . By rearranging the equation, you solve for n, which is n=(PV)/(RT)

P= 28.3 atm

V=0.193 L

R= 0.08206 L atm mol^-1 K^-1

T= 24.5+273.15= 297.65 K

Plugging the values in,

n=(28.3 atm x 0.193 L)/(0.08206 L atm mol^-1 K^-1 x 297.65 K)

n= 0.224 moles of oxygen

3. At STP, there are 22.4 L of gas for every mole of gas present. So 6.4 moles of oxygen would mean that there are:

6.4 mol x 22.4 L= 143.36 L oxygen gas

5. You have to use the ideal gas law: PV=nRT where P is pressure in atm, V is volume in liters, n is number of moles, R is the constant 0.08206 L atm mol^-1 K^-1, and T is the temperature in Kelvins where K=degrees celsius+273.15 . By rearranging the equation, you solve for P, which is P=(nRT)/V

n= 0.72 g converting to moles, divide by molar mass of oxygen gas: 0.72 g/32g= 0.0225 moles

V=9.3 L

R= 0.08206 L atm mol^-1 K^-1

T= 23.0+273.15= 296.15 K

Plugging the values in,

P=(0.0225 moles x 0.08206 L atm mol^-1 K^-1 x 296.15 K)/ 9.3 L

P= 0.059 atm

10. Ideal gas law again using the same equation as 5 above: You have to use the ideal gas law: PV=nRT where P is pressure in atm, V is volume in liters, n is number of moles, R is the constant 0.08206 L atm mol^-1 K^-1, and T is the temperature in Kelvins where K=degrees celsius+273.15 . By rearranging the equation, you solve for P, which is P=(nRT)/V

n= 0.108 mol

R=0.08206 L atm mol^-1 K^-1

T=20.0+273.15= 293.15 K

V= 0.505 L

Plugging the values in,

P=(0.108 mol x 0.08206 L atm mol^-1 K^-1 x 293.15 K)/0.505 L

P= 5.14 atm

11. You have to use the ideal gas law: PV=nRT where P is pressure in atm, V is volume in liters, n is number of moles, R is the constant 0.08206 L atm mol^-1 K^-1, and T is the temperature in Kelvins where K=degrees celsius+273.15 . By rearranging the equation, you solve for Y, which is T=(PV)/(nR)

P= 0.988 atm

V= 1.20 L

n= 0.0470 mol

R=0.08206 L atm mol^-1 K^-1

Plugging the numbers in,

T=(0.988 atm x 1.20 L)/(0.0470 mol x 0.08206 L atm mol^-1 K^-1)

T= 307 K

4 0

3 years ago

PLSS HELP ASAP PLSS

Zepler [3.9K]

molar concentration of Na⁺ ions = 3 M

molar concentration of CO₃⁻ ions = 1.5 M

First the water will solvate the sodium carbonate (Na₂CO₃).

Second the 80 mL of water added will dilute the first solution.

Explanation:

When you dissolve the Na₂CO₃ in water, the following solvation process takes place:

Na₂CO₃ (s) + H₂O (l) → 2 Na⁺ (aq) + CO₃⁻ (aq)

To find the final concentration of Na₂CO₃ solution we use the following formula:

concentration (1) × volume (1) = concentration (2) × volume (2)

concentration (2) = concentration (1) × volume (1) / volume (2)

concentration of Na₂CO₃ solution = 2.5 M × 120 mL / 200 mL

concentration of Na₂CO₃ solution = 1.5 M

molar concentration = number of moles / volume (L)

number of moles = molar concentration × volume (L)

number of moles of Na₂CO₃ = 1.5 M × 0.2 L = 0.3 moles

Knowing the solvation process we devise the following reasoning:

if 1 mole of Na₂CO₃ produces 2 moles of Na⁺ ions and 1 mole of CO₃⁻ ions

then 0.3 moles of Na₂CO₃ produces X moles of Na⁺ ions and Y mole of CO₃⁻ ions

X = (0.3 × 2) / 1 = 0.6 moles of Na⁺ ions

Y = (0.3 × 1) / 1 = 0.3 moles of CO₃⁻ ions

molar concentration = number of moles / volume (L)

molar concentration of Na⁺ ions = 0.6 / 0.2 = 3 M

molar concentration of CO₃⁻ ions = 0.3 / 0.2 = 1.5 M

Learn more about:

molar concentration

brainly.com/question/14124542

#learnwithBrainly

6 0

3 years ago