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3 years ago

Neutral atoms of a specific element can have different numbers of which?

Chemistry

2 answers:

Solnce55 [7]3 years ago

7 0

The correct answer is protons and electrons

soldier1979 [14.2K]3 years ago

3 0

Protons and elections! That’s correct!

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When hydrogen peroxide (H2O2) is used in rocket fuel, it produces water and oxygen (O2): Can someone help with parts B and C?

Paladinen [302]

Answer:

Explanation: A foam forms when bubbles of a gas are trapped in a liquid or solid. In this case oxygen is generated when hydrogen peroxide breaks down into oxygen and water on contact with catalase, an enzyme found in liver. Enzymes are special protein molecules that speed up chemical reactions.

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3 years ago

What type of thermal transfer is holding on to an ice cube?

telo118 [61]

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3 years ago

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Gold and helium are examples of a(n)

kogti [31]

I guess examples of solid and gas???? You have to be more descriptive.....

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3 years ago

How many kJ of heat do you need to raise the temperature of 200 g of Aluminum from 80 °C to 100 °C?

marta [7]

Answer:

0.01

Explanation:

100 -80=20

200/20=10/1000=0.01kj

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2 years ago

Calculate Horxn for the following reaction:H3AsO4(aq) + 4 H2(g) --> AsH3(g) + 4 H2O(l)(Hof [AsH3(g)] = 66.4 kJ/mol; Hof [H

Juli2301 [7.4K]

Answer:

The Standard enthalpy of reaction: $\Delta H_{r}^{\circ } = (-172.2) \, kJ$

Explanation:

Given- Standard Heat of Formation:

$\Delta H_{f}^{\circ } [H_{3}AsO_{4}(aq)]$ = -904.6 kJ/mol

$\Delta H_{f}^{\circ } [H_{2}(g)]$ = 0 kJ/mol,

$\Delta H_{f}^{\circ } [AsH_{3}(g)]$ = +66.4 kJ/mol

$\Delta H_{f}^{\circ } [H_{2}O(l)]$ = -285.8 kJ/mol

Given chemical reaction: H₃AsO₄(aq) + 4H₂(g) → AsH₃(g) + 4H₂O(l)

The standard enthalpy of reaction: $\Delta H_{r}^{\circ }$ = ?

To calculate the Standard enthalpy of reaction ( $\Delta H_{r}^{\circ }$ ), we use the equation:

$\Delta H_{r}^{\circ } = \sum \nu .\Delta H_{f}^{\circ }(products)-\sum \nu .\Delta H_{f}^{\circ }(reactants)$

$\Delta H_{r}^{\circ } = [1 \times \Delta H_{f}^{\circ } [AsH_{3} (g)] + 4 \times \Delta H_{f}^{\circ } [H_{2}O(l)]] - [1 \times \Delta H_{f}^{\circ } [H_{3}AsO_{4}(aq)] + 4 \times \Delta H_{f}^{\circ } [H_{2}(g)]$

$\Rightarrow \Delta H_{r}^{\circ } = [1 \times (+66.4\,kJ/mol) + 4 \times (-285.8\,kJ/mol) ] - [1 \times (-904.6\,kJ/mol) + 4 \times (0\,kJ/mol)]$

$\Rightarrow \Delta H_{r}^{\circ } = [-1076.8\, kJ] - [-904.6\,kJ]$

$\Rightarrow \Delta H_{r}^{\circ } = (-172.2 \, kJ)$

Therefore, the Standard enthalpy of reaction: $\Delta H_{r}^{\circ } = (-172.2) \, kJ$

5 0

3 years ago