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3 years ago

I’m extremely stuck on this, please help

Chemistry

1 answer:

nataly862011 [7]3 years ago

5 0

Answer:

ice: 2,100 J/(kg·K)

water: 4,200 J/(kg·K)

water vapor: 2,000 J/(kg·K)

basalt: 840 J/(kg·K)

granite: 790 J/(kg·K)

aluminum: 890 J/(kg·K)

iron: 450 J/(kg·K)

copper: 380 J/(kg·K)

lead: 130 J/(kg·K)

Explanation:

Specific heat is the amount of thermal energy you need to supply to a sample weighing 1 kg to increase its temperature by 1 K.

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Determine the root-mean square speed of CO2 molecules that have an average kinetic energy of 4.2 x10-21 J per molecule.

strojnjashka [21]

Determine the root-mean-square sped of CO2 molecules that have an average Kinetic Energy of 4.21x10^-21 J per molecule. Write your answer to 3 sig figs.

E = 1/2 m v^2

If you substitute into this formula, you will get out the root-mean-square speed.

If energy is Joules, the mass should be in kg, and the speed will be in m/s.

1 mol of CO2 is 44.0 g, or 4.40 x 10^1 g or 4.40 x 10^-2 kg.

If you divide this by Avagadro's constant, you will get the average mass of a CO2 molecule.

4.40 x 10^-2 kg / 6.02 x 10^23 = 7.31 x 10^-26 kg

So, if E = 1/2 mv^2

v^2 = 2E/m = 2 (4.21x10^-21 J)/7.31 x 10^-26 kg = 115184.68
Take the square root of that, and you get the answer 339 m/s.

8 0

3 years ago

2.What are variables used to describe weather?

Studentka2010 [4]

The answer is, All of the above

4 0

2 years ago

What is the IUPAC name Of CH3-CH2-CH2-CH=O I COOH

Blizzard [7]

Answer:

Explanation:

It is Butanoic Acid

8 0

2 years ago

Read 2 more answers

2) what is the mass of 6.02 x 1023 atoms of arsenic?

zzz [600]

Data:
Arsenic Molar Mass = 74,9216 ≈ 75 u (atomic mass unit)

Solving:

1 mole of arsenic → 75g ------------ 6,02*10²³ molecules
..................................X -------------- 1 molecule

6,02*10²³X = 75
$x = \frac{75}{6,02*10^{23}}$
$\boxed{x \approx 1,24*10^{24}grams}$

6 0

2 years ago

The free energy change for the following reaction at 25 °C, when [Cr3+] = 1.32×10-3 M and [Fe3+] = 1.14 M, is 131 kJ: Cr3+(1.32×

larisa [96]

Answer:

E°cell = - 1.3575 V

This reaction is spontaneous in the reverse direction

Explanation:

The given cell reaction:

Cr³⁺(1.32 × 10⁻³ M) + Fe²⁺(aq) → Cr²⁺(aq) + Fe³⁺(1.14 M)

The given Gibbs free energy: ΔG = 131 kJ = 131 × 10³ J (∵ 1 kJ = 10³ J)

As we know,

ΔG = - n F E°cell

Here, n - the number of moles of electrons transferred = 1

F - Faraday constant = 96500

E°cell - cell potential = ?

$\therefore E^{\circ }_{cell} = -\frac{\Delta G}{n \: F} = -\frac{131\times 10^{3}\, J}{1\, mol\times96500 \, C.mol^{-1}}$

$\Rightarrow E^{\circ }_{cell} = -1.3575\, V$

For a given chemical reaction if-

1. ΔG = negative and E°cell = positive

⇒ The reaction is spontaneous and proceeds spontaneously in the forward direction.

2. ΔG = positive and E°cell = negative

⇒ The reaction is non-spontaneous and proceeds spontaneously in the reverse direction.

Since, for this chemical reaction: 

Cr³⁺(1.32 × 10⁻³ M) + Fe²⁺(aq) → Cr²⁺(aq) + Fe³⁺(1.14 M)

ΔG = + 131 × 10³ J ⇒ positive

and, E°cell = - 1.3575 V ⇒ negative

Therefore, this reaction is spontaneous in the reverse direction.

6 0

3 years ago