The beginning expansion of the big bang happened relatively slowly compared to how it is expanding now.

ozzi

Answer:

an ideal gas does not exist except as a conceptual notion, an ideal. Physicists and chemists idealized the behaviour of real gases so that they could explain these phenomena. Under conditions of low pressure and high temperature, all gases behave like real gases, even gases such as UF6 .

5 0

3 years ago

You have a sample of each of the following five metals, with the mass and density

Sindrei [870]

Answer:

E) Silver, mass = 420 g, d = 10.5 g/cm.

Explanation:

Hello,

In this case, since the density is defined by:

$\rho =\frac{m}{V}$

Given the mass and density, we compute the volume via:

$V=\rho *m$

Thus, for each vase we have:

A) $V=135g*2.7g/cm^3=364.5cm^3$

B) $V=305g*8.92g/cm^3=2720.6cm^3$

C) $V=240g*7.86g/cm^3=1886.4cm^3$

D) $V=75g*1.74g/cm^3=130.5cm^3$

E) $V=420g*10.5g/cm^3=4410cm^3$

In such a way, the largest volume corresponds to E) Silver, mass = 420 g, d = 10.5 g/cm.

Best regards.

7 0

3 years ago

For the reaction 3h2(g) + n2(g) 2nh3(g), kc = 9.0 at 350°c. calculate g° at 350°c.

miss Akunina [59]

When ΔG° is the change in Gibbs free energy

So according to ΔG° formula:

ΔG° = - R*T*(㏑K)

here when K = [NH3]^2/[N2][H2]^3 = Kc

and Kc = 9

and when T is the temperature in Kelvin = 350 + 273 = 623 K

and R is the universal gas constant = 8.314 1/mol.K

So by substitution in ΔG° formula:

∴ ΔG° = - 8.314 1/ mol.K * 623 K *㏑(9)

= - 4536

4 0

3 years ago

How much heat is required to warm 50.0 g of ice from -10.0oC to 0.00oC, melt the ice, warm the water from 0.00oC to 100.0oC, boi

ludmilkaskok [199]

The total heat required to convert the ice to steam is 155,000 J.

The given parameters:

Mass of the ice, m = 50 g
Initial temperature of the ice, t = -10 ⁰C
Final temperature of the ice, T = 0⁰C, 100⁰C and 120⁰C
Specific heat capacity of water = 4.184 J/g⁰C
Heat of fusion of ice, = 333.55 J/g
Heat of vaporization, = 2,230 J/g

The heat required to raise the temperature to 0⁰C is calculated as;

$Q = mc\Delta t\\\\Q_1 = 50 \times 4.184 \times (0 - (-10))\\\\Q_1 = 2092 \ J$

The heat required to melt the ice is calculated as follows;

$Q_2 = mL_f\\\\Q_2 = 50 \times 333.55 \\\\Q_2 = 16,677.5 \ J$

The heat raise the temperature to 100⁰C is calculated as;

$Q_3 = 50 \times 4.184 \times (100 - 0)\\\\Q_3 = 20,920 \ J$

The heat required to boil the water is calculated as follows;

$Q_4 = mL_v\\\\Q_4 = 50 \times 2230\\\\4_4 = 111,500 \ J$

The heat raise the temperature to 120⁰C is calculated as;

$Q_5 = 50 \times 4.184 \times (120 - 100)\\\\Q_5 = 4,184 \ J$

The total heat required is calculated as follows;

$Q_t = Q_1 + Q_2 + Q_3 + Q_4 + Q _5 \\\\Q_t = 2092 + 16,677.5 + 20,920 + 111,500 + 4,184\\\\Q_t = 155,373.5 \ J\\\\Q_t \approx 155,000 \ J$

Learn more about heat capacity here: brainly.com/question/16559442

4 0

3 years ago

What factors affect the radius of an atom?

Diano4ka-milaya [45]

Answer:

Atomic radius is determined as the distance between the nuclei of two identical atoms bonded together. The atomic radius of atoms generally decreases from left to right across a period. The atomic radius of atoms generally increases from top to bottom within a group.

8 0

3 years ago