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3 years ago

The physical properties of a material depend on its _________.

Chemistry

1 answer:

ira [324]3 years ago

5 0

Answer:

color, shape, texture, odor, sound, malleability, ductility, volume, mass, density, boiling point, melting point, viscosity, hardness, conductility.

Explanation:

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Calculate the concentration of acetic acid, HAc, and acetate ion, Ac−, in a 0.25M acetate buffer solution with pH = 5.36. "0.25M

Neporo4naja [7]

Answer:

[HAc] = 0.05M

[Ac⁻] = 0.20M

Explanation:

The Henderson-Hasselbalch formula for the acetic acid buffer is:

pH = pka + log₁₀ [Ac⁻] / [HAc]

Replacing:

5.36 = 4.76 + log₁₀ [Ac⁻] / [HAc]

3.981 = [Ac⁻] / [HAc] (1)

Also, as total concentration of buffer is 0.25M it is possible to write:

0.25M = [Ac⁻] + [HAc] (2)

Replacing (2) in (1)

3.981 = 0.25M - [HAc] / [HAc]

3.981 [HAc] = 0.25M - [HAc]

4.981 [HAc] = 0.25M

[HAc] = 0.05M

Replacing this value in (2):

0.25M = [Ac⁻] + 0.05M

[Ac⁻] = 0.20M

I hope it helps!

7 0

4 years ago

A gas in a piston–cylinder assembly undergoes a compression process for which the relation between pressure and volume is given

m_a_m_a [10]

Answer:

$A=69.8\frac{bar}{m^6}\\\\ B=0.00302bar*m^6$

2. $W=-8.2kPa$

Explanation:

Hello,

1. In this case, for the given p-V equation, one could use the two states to form a 2x2 linear system of equations in terms of A and B:

$\left \{ {{0.1^2A+0.1^{-2}B=1} \atop {0.04^2A+0.04^{-2}B=2}} \right.$

$\left \{ {{0.01A+100B=1} \atop {0.0016A+625B=2}} \right$

Whose solution by any method for solving 2x2 linear system of equations (elimination, reduction or substitution) is:

$A=69.8\frac{bar}{m^6}\\\\ B=0.00302bar*m^6$

2. Now, for us to compute the work, we must first compute n, as the power relating the pressure and volume for this process:

$P_1V_1^n=P_2V_2^n\\\\\frac{P_1}{P_2}=(\frac{V_2}{V_1} )^n\\\\\frac{1bar}{2bar}= (\frac{0.04m^3}{0.1m^3} )^n\\\\0.5=0.4^n\\\\n=\frac{ln(0.5)}{ln(0.4)} =0.7565$

Now, we compute the work:

$W=\frac{P_2V_2-P_1V_1}{1-n} =\frac{2bar*0.04m^3-1bar*0.1m^3}{1-0.7565} \\\\W=-0.082bar*m^3*\frac{1x10^2kPa}{1bar}\\ \\W=-8.2kPa$

Regards.

8 0

4 years ago

The following equation shows the equilibrium in an aqueous solution of ammonia: NH3(aq)+H2O(l)⇌NH4+(aq)+OH−(aq)NH3(aq)+H2O(l)⇌NH

yarga [219]

Answer:

c) H2O and OH−

Explanation:

Acids are the species which furnish hydrogen ions in the solution or is capable of forming bonds with electron pair species as they are electron deficient species.

When an acid donates a proton, it changes into a base which is known as its conjugate base.

Bases are the species which furnish hydroxide ions in the solution or is capable of forming bonds with electron deficient species as they are electron rich species. When a base accepts a proton, it changes into a acid which is known as its conjugate acid.

The acid and the base which is only differ by absence or presence of the proton are known as acid conjugate base pair.

Thus, for the reaction,

$NH_3+H_2O\rightleftharpoons Nh_4^++OH^-$

The base is $NH_3$ and the conjugate acid of the base is $NH_4^+$ .

Also, The base is $OH^-$ and the conjugate acid of the base is $H_2O$ .

Correct option is :- c) H2O and OH−

8 0

3 years ago

When 16 g of methane (CH4) and 32 g of oxygen (O2) reacted to produce carbon dioxide and water, 11 g of carbon dioxide was produ

Aliun [14]

Answer:

Percent yield = 50%

Explanation:

Given data:

Mass of CH₄ = 16 g

Mass of O₂ = 32 g

Mass of CO₂ = 11 g

Percent yield of CO₂ = ?

Solution:

Chemical equation:

CH₄ + 2O₂ → CO₂ + 2H₂O

Number of moles of CH₄:

Number of moles = mass/ molar mass

Number of moles = 16 g /16 g/mol

Number of moles = 1 mol

Number of moles of O₂:

Number of moles = mass/ molar mass

Number of moles = 32 g /32 g/mol

Number of moles = 1 mol

Now we will compare the moles of CO₂ with both reactant.

O₂ : CO₂

2 : 1

1 : 1/2×1= 0.5 mol

CH₄ : CO₂

1 : 1

Number of moles of CO₂ produced by oxygen are less so it will limiting reactant.

Theoretical yield:

Mass of CO₂:

Mass = number of moles × molar mass

Mass = 0.5 mol × 44 g/mol

Mass = 22 g

Percent yield:

Percent yield = actual yield / theoretical yield × 100

Percent yield = 11 g/ 22 g × 100

Percent yield = 50%

3 0

3 years ago

1, 2 and 3 ........

Orlov [11]

2.) Average atomic mass =Σ (abundance x molar mass) /100 = (12.64 x 302.04 + 18.23 x 304.12 + 69.13 x 305.03) /100 =304.486 u(Dalton) . This is avg atomic mass.

8 0

4 years ago