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hammer [34]
3 years ago
13

What did Rutherford’s nuclear atomic model not explain?

Chemistry
1 answer:
statuscvo [17]3 years ago
4 0

Answer:

It did not explain/ support the existence of the Nucleus as another subatomic particle in the atomic nucleus.

Explanation:

The proof was provided by another English scientist, James Chadwick.

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1- What do greenhouse gases do in our atmosphere? a. They absorb radiation given off by the Earth b They block harmful radiation
zavuch27 [327]

Answer: A. They absorb radiation given off by the earth.

Explanation: Green house gases are gases that have the capability of trapping the heat energy from the sun in our environment. These special attribute of these gases is what keeps our environment warm and sustain life as we know it. Example of Green House Gases include: carbon dioxide, water vapour and methane.

8 0
4 years ago
Read 2 more answers
What is the most important requirement for all living things? water carbon dioxide light vitamins
Sidana [21]
Water. All organisms that depend on oxygen need water to live.
5 0
3 years ago
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Convert to moles:<br> 100.0g Ca3(PO4)2
salantis [7]

Answer:

0.322 moles

Explanation:

Given Mass, m = 100 g

The molar mass of Ca₃(PO₄)₂

Ca₃(PO₄)₂ = (3 x 40.08) + (2 x 30.97) + (8 x 16.00)

M = 310.18 g/mol

Let there are n number of moles,

n = given mass/ molar mass

n=\dfrac{100 }{310.18 }\\\\n=0.322\ mol

So, there are 0.322 moles.

6 0
3 years ago
At 400 K, the rate of decomposition of a gaseous compound initially at a pressure of 12.6 kPa, was 9.71 Pa s-1 when 10.0 per cen
Neporo4naja [7]

Answer:

The order of the reaction with respect to the gas = 2

Explanation:

Let the original gas pressure be [G₀]

Initial rate of reaction is given as

r = k [G₀]ⁿ

When 10% had reacted, amount of gas left = [0.9G₀], r = 9.71 Pa/s

r = k [0.9G₀]ⁿ = 9.71 (eqn 1)

when 20% had reacted, amount of gas left = [0.8G₀], r = 7.67 Pa/s

r = k [0.8G₀]ⁿ = 7.67 (eqn 2)

Dividing (eqn 1) by (eqn 2)

(9.71/7.67) = [0.9/0.8]ⁿ

1.266 = 1.125ⁿ

1.125ⁿ = 1.266

Take natural logarithms of both sides

n (In 1.125) = In 1.266

n = 0.236/0.118

n = 2.

7 0
3 years ago
A balloon that can hold 85 L of air is inflated with 7.056 grams of H2 gas at a pressure of 101.3 kPa. What is the temperature,
evablogger [386]
<h2>Answer:</h2>

Temperature is 258.32°C

<h2>Explanation:</h2>

Using the ideal gas equation;

PV = nRT        --------------(i)

Where;

P = Pressure of the gas

V = Volume of the gas

n = number of moles of the gas

R = Gas constant = 8.31 J/mol · K

T = Temperature

<em><u>Given:</u></em>

mass of H₂ gas = 7.056 grams

Volume of the gas = 85L = 8.5 x 10⁻³m³

Pressure of the gas = 101.3kPa = 101.3 x 10³Pa = 1.013 x 10⁵Pa

<em><u>Steps:</u></em>

(i) Using the mass of the gas, calculate the number of moles using the relation:

n = m / M         ----------------- (ii)

Where;

m = mass of H₂ = 7.056g

M = Molar mass of H₂ = 1g/mol

<em>Substitute these values into equation (ii) as follows:</em>

n = 7.056g / (1g/mol)

n = 7.056mol

(ii) Now calculate the temperature of the balloon by substituting the necessary values into equation (i)

(1.013 x 10⁵Pa)(8.5 x 10⁻³m³) = (7.056mol) (8.31 J/mol · K)(T)

T = (1.013 x 10⁵Pa)(8.5 x 10⁻³m³) ÷ (7.056mol) (8.31 J/mol · K)

<em>Solving the above gives</em>

T = 14.68K

<em>Convert this to Celsius </em>

T = 273 - 14.68

T = 258.32°C

8 0
3 years ago
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