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3 years ago

What factors could have affected your results?

Chemistry

1 answer:

AleksandrR [38]3 years ago

8 0

Answer:

See below

Step-by-step explanation:

heat gained by metal + heat lost by water = 0

m₁C₁ΔT₁ + m₂C₂ΔT₂ = 0

C₁ = -(m₂C₂ΔT₂)/(m₁ΔT₁)

The factors determining C₁ are

mass of water
temperature change of water (T_f - Ti)
mass of metal
temperature change of metal (T_f - Ti)

Any factor that makes the numerator higher or the denominator lower than what you thought, will give a calculated C₁ that is too high (and vice versa).

The major sources of uncertainty are probably in determining the temperatures, especially the initial and final temperatures of the metal. However, you will have to decide what the principal factors were in your experiment.

For example, did the metal have a chance to cool during the transfer to the calorimeter? How easy was it to determine the equilibrium temperature, etc?

Factors Affecting the Calculation of Specific Heat Capacity

Water Water

Mass less than thought Mass more than thought

Ti lower Ti higher

T_f higher T_f lower

Metal Metal

Mass more than thought Mass less than thought

Ti higher Ti lower

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Is this molecule polar or nonpolar?

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3 years ago

You have 100 g of Pb(NO3)2. How many moles is this?

topjm [15]

Answer:

0.302 moles

Explanation:

Data given

Mass of Pb(NO₃)₂ = 100 g

Moles of Pb(NO₃)₂ = ?

Solution:

To find mole we have to know about molar mass of Pb(NO₃)₂

So,

Molar mass of Pb(NO₃)₂ = 207 + 2[14 + 3(16)]

= 207 + 2[14 + 48]

= 207 + 124

Molar mass of Pb(NO₃)₂ = 331 g/mol

Formula used :

no. of moles = mass in grams / molar mass

Put values in above formula

no. of moles = 100 g / 331 g/mol

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3 years ago

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3 years ago

Read 2 more answers

Titanium has an HCP crystal structure, a c/a ratio of 1.669, an atomic weight of 47.87 g/mol, and a density of 4.51 g/cm3. Compu

IrinaK [193]

Answer : The atomic radius for Ti is, $1.45\times 10^{-8}cm$

Explanation :

Atomic weight = 47.87 g/mole

Avogadro's number $(N_{A})=6.022\times 10^{23} mol^{-1}$

First we have to calculate the volume of HCP crystal structure.

Formula used :

$\rho=\frac{Z\times M}{N_{A}\times V}$ .............(1)

where,

$\rho$ = density = $4.51g/cm^3$

Z = number of atom in unit cell (for HCP = 6)

M = atomic mass = 47.87 g/mole

$(N_{A})$ = Avogadro's number

V = volume of HCP crystal structure = ?

Now put all the values in above formula (1), we get

$4.51g/cm^3=\frac{6\times (47.87g/mol)}{(6.022\times 10^{23}mol^{-1}) \times V}$

$V=1.06\times 10^{-22}cm^3$

Now we have to calculate the atomic radius for Ti.

Formula used :

$V=6R^2c\sqrt{3}$

Given:

c/a ratio = 1.669 that means, c = 1.669 a

Now put (c = 1.669 a) and (a = 2R) in this formula, we get:

$V=6R^2\times (1.669a)\sqrt{3}$

$V=6R^2\times (1.669\times 2R)\sqrt{3}$

$V=(1.669)\times (12\sqrt{3})R^3$

Now put all the given values in this formula, we get:

$1.06\times 10^{-22}cm^3=(1.669)\times (12\sqrt{3})R^3$

$R=1.45\times 10^{-8}cm$

Therefore, the atomic radius for Ti is, $1.45\times 10^{-8}cm$

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3 years ago

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